Download ID_260_Equilibria in biological syste_English_sem_1

1.
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Reversible is all reaction except:
N2O4(g)  2NO2(g);
2KClO3 (s)2KCl(s) + 3O2(g);
N2 (g) + 3H2(g)  2NH3(g);
N2(g) + O2(g)  2NO(g);
C2H4 (g) + H2(g)  C2H6(g).
Irreversible reaction is:
CaCO3 (s)CaO(s) + CO2(g);
N2O4(g)  2NO2(g);
N2 (g) + 3H2(g)  2NH3(g);
N2(g) + O2(g)  2NO(g);
C3H6 (g) + H2(g)  C3H8(g).
The kinetic energy that reactant molecules must have allow them to reach the transition state so that a
reaction can occur.
Heat effect reaction;
Potential energy;
Activation reaction;
Enthalpy;
Free Gibbs’ energy.
The time required for half of that reactant to the converted into product.
Heat effect reaction.
Molecularity;
Time of reaction;
Order reaction;
Half-life a reactant;
The equation:
for this reaction
is:
Rate law equation;
van’t Hoff law equation;
Rate equation;
Chemical equilibrium constant;
Arhenius’ law equation.
The study of rates and mechanisms of chemical reactions and of the factors on which they depend is:
Thermodynamics;
Electrochemistry;
Colloidal chemistry;
Chemical kinetics;
Gravimetric analysis.
"k" in rate law equation
Rate constant;
Mass-action expression;
Chemical equilibrium constant;
Rate;
Temperature reaction.
is:
A.
B. *
C.
D.
E.
10.
A.
B.
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D.
E.
11.
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B.
C.
D.
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А system usually consists of а definite amount of one or more substances and is separated from the
surroundings by а real or imaginary boundary through which matter and energy can flow from the
system to the surroundings or vice versa:
Exogenous and endogenous;
One, two, three compounds;
Homogenous and heterogeneous;
Isolated, opened, closed.
Reversible and irreversible.
It is used stable temperature and pressure for the most processes in chemical technology. What name
is process?
Isochoric - Isothermel;
Isobar - Isothermic;
Isobar - Isochoric;
Isochoric - Adiabatic;
Isothermal - Adiabatic.
Standard state of a system is state when:
101,3 kPa, 0 0K.
101,3 kPa, 273 0K.
101,3 kPa, 298 0K.
50 kPa, 273 0K.
50 kPa, 298 0K.
The state of the system, when it composition and function does not change in time is called:
Isochoric.
Adiabatic
Isothermal.
Isobar.
Equilibrium.
12.
A. *
B.
C.
D.
E.
The standard formation of combustion (ΔН°formation) equal zero for such compound:
O2, Н2.
СО2, Н2О.
NO, NH3.
P2O3, PH3.
NO2, N2H4.
13.
A.
B.
C. *
For an isochoric process the Heat effect equal:
Zero.
Change of enthalpy.
Change of internal energy.
D.
E.
Change of entropy.
Change of free Gibbs’s energy.
14.
A.
B.
C.
D. *
The first law equation is:
dH = dQ + dE
Q=A+W
Q = dHW
Q=U+W
8.
A.
B.
C.
D. *
E.
9.
E.
15.
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B.
C.
D.
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B.
C.
D. *
E.
S = dG + W
The concept “Total general of energy is stable in all isolated system” is:
First law of thermodynamics.
Second law of thermodynamics.
Third law of thermodynamics.
Hess’s law.
Kirchhoff’s law.
Heat effect of reaction oxidation 1 mole of compound at standard state is called:
Standard enthalpy of dissolved.
Standard enthalpy of neutralization
Standard enthalpy of formation.
Standard enthalpy of combustion.
Standard enthalpy of precipitation.
17.
A.
B.
C. *
Thermodynamics systems are classified by amount of phases into:
Exogenous and endogenous.
Solid, liquid, gas.
Homogeneous and heterogeneous.
D.
E.
18.
A.
B.
C.
D.
E. *
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A.
B. *
C.
D.
E.
20.
A.
Isolated, opened, closed
Reversible and irreversible.
When temperature is stable this process is called?
Isolated;
Isobaric;
Isochoric.
Adiabatic;
Isothermic.
Normal state is state when:
101,3 kPa, 0 0K.
101,3 kPa, 273 0K.
101,3 kPa, 298 0K.
50 kPa, 273 0K.
50 kPa, 298 0K.
Measure of randomness or disorder of the system is:
Heat.
B.
C.
D. *
E.
21.
A.
B.
C. *
D.
E.
Work.
Enthalpy.
Entropy.
Internal energy.
The equation for pressure-volume work at isobar expansion is:
W= VS
W= pQ
W = p ΔV
W=nRTln(V2/V1)
W=nRT (V2/V1)
22.
A.
B.
C.
D. *
Temperature dependence of heat effect of reaction is studied such law:.
First law of thermodynamics.
Second law of thermodynamics.
Third law of thermodynamics.
Kirchhoff’s law.
E.
23.
A.
B. *
Hess’s law.
C.
D.
E.
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B.
C.
D.
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B.
C.
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C.
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Homogenous;
Isolated;
Opened.
If system can exchange both matter and energy with the surroundings, it is called:
Exogenous;
Closed
Homogenous;
Isolated;
Opened.
If а system can neither exchange matter or energy with the surroundings, it is called
Exogenous;
Closed
Homogenous;
Isolated;
Opened
Closed thermodynamics systems are systems, which can exchange with the surroundings:
Matter.
Energy.
Both matter and energy.
Temperature.
Neither exchange matter nor energy.
Opened thermodynamics systems are systems, which can exchange with the surroundings:
Matter.
Energy.
Both matter and energy
Temperature.
Neither exchange matter nor energy.
The concept “The total amount of heat evolved or absorbed in a reaction depends only upon the
nature of the initial reactants and that of the final products and does not depend upon the path by
which this change is brought about” is:
First law of thermodynamics.
Second law of thermodynamics.
Third law of thermodynamics.
Hess’s law.
Kirchhoff’s law.
A.
B.
C.
D. *
E.
If а system can exchange only energy with the surroundings but not matter, it is called:
Exogenous;
Closed
29.
A.
B.
C.
D. *
E.
In spontaneous processes the Gibbs’s energy is:
Maximal.
Zero.
Minimal.
Negative.
Positive
30.
A.
E.
The spontaneous processes are in such circumstances:
G≥0, S<0.
G0, S  0.
G=0, S=0.
G<0, S>0.
G>0, S<0.

The non spontaneous processes are in such circumstances:
G0, S<0.
G0, S  0.
G=0, S=0.
G<0, S>0.
G>0, S<0.
The equilibrium state is in such circumstances:
G0, S<0.
G0, S  0.
G=0, S=0.
G>0, S<0.
G<0, S>0.
33.
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C.
D.
E.
34.
Chemical kinetics studies:
Properties of solutions;
Speed of chemical reactions and its dependence on the different factors;
Buffer systems of blood;
pH of solutions;
Oxidation- reduction reactions.
If all reagent and products of reaction are in same phase, this reaction is called:
A. *
B.
C.
D.
E.
35.
A. *
B.
C.
D.
Homogeneous
Single-phased
Multi-phased
Heterogeneous
Different-phased
Rate constant is:
k = υ if concentration of reagents equal one unit;
Degree of precipitation;
Mass constant;
k = υ if concentration of reagents equal 0.1;
B.
C.
D. *
E.
31.
A.
B.
C.
D.
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32.
A.
B.
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D.
A.
B. *
C.
D.
E.
k = υ if concentration of reagents equal 10.
Heterogeneous system is:
System which consists of one phase;
System which consists of two or more phases;
Contain liquid;
System which consists of a single phase;
System in which is distilled water .
All factors influence for rate of reaction except:
Concentration of the reactants.
Temperature.
Presence of Catalyst.
Surface area of the reactants.
Color of indicator.
Rate of chemical reaction is:
The change in the concentration of any one of the reactants or products per unit of time;
The change of the coloring of indicator;
The change of volume;
The change of pH value;
The change of temperature.
Reversible system is:
System which consists of one phase;
System which consists of two more phases;
Consist liquid and gas phases;
System which consists of five phases;
System which is carried out infinitestimally.
Branch of chemistry which deals with the study of the speeds or the rates f chemical reactions, the
factors affecting the rates of the reactions and the mechanism by which the reactions proceed is:
Thermodynamics.
Chemical kinetics.
Analytical chemistry;
Electrochemistry;
Inorganic chemistry.
41.
A.
B.
C.
D. *
If all reagent and products of reaction are in different phases, this reaction is called:
Homogeneous
Single-phased
Different-phased
Heterogeneous
E.
Similar.
42.
A. *
Vant-Goff rule:
Rate of homogeneous chemical reaction is increase in two - four times when temperature is increase
on 10 0С.
Total mass of chemical reaction reagent equal total mass of products;
Energy is stable.
Properties of elements, and they derivative are depended on atoms weight;
E.
36.
A.
B. *
C.
D.
E.
37.
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B.
C.
D.
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A. *
B.
C.
D.
E.
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B.
C.
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40.
B.
C.
D.
E.
43.
A.
B.
C. *
D.
E.
Heat effect of reaction is constant, when is formed same reagents.
An empirical quantity, and obtained from the experimental rate law is:
Rate constant;
Molecularity;
Reaction order;
Mass constant;
Stoichiometric coefficient.
44.
A.
B. *
C.
D.
E.
An elementary reaction proposed as an individual step in а mechanism is:
Rate constant;
Molecularity;
Reaction order;
Mass constant;
Stoichiometric coefficient.
45.
A. *
B.
C.
D.
E.
For rate constant influence all factors except:
Concentration of the reactants.
Temperature.
Pressure.
Surface area of the reactants.
Nature of reagents.
46.
A.
B.
What factors are influence for rate constant?
Concentration of the reactants.
Indicator.
C.
D.
E. *
Dispersed phase.
Surfactant.
Nature of reagents.
47.
A. *
B.
C.
D.
E.
48.
What factors influence for rate of reaction?
Concentration of the reactants.
Indicator.
Dispersed phase.
Surfactant
A.
B.
C. *
D.
E.
49.
A. *
B.
Surface tension.
Rate law equation for reaction: 2 SO2 (g) + O2 (g) 2 SO3 (g) is:
= k [SO3]2 [O2].
= k 2[SO2] [O2].
= k [SO2]2 [O2].
= k [O2].
= k [SO3].

Rate law equation for reaction: 2 SO3 (g)  2 SO2 (g) + O2 (g) is:
= k [SO3]2.
= k 2[SO2] [O2].
C.
D.
E.
50.
A.
B. *
C.
D.
E.
51.
A.
B.
C. *
D.
E.
52.
A.
B.
C.
D.
E. *
53.
A. *
B.
C.
D.
E.
54.
A.
B. *
C.
D.
E.
55.
A. *
B.
C.
D.
E.
56.
A.
= k [SO2]2 [O2].
= k [O2].
= k [SO2].
Rate law equation for reaction: 2 NO (g) + O2 (g) 2 NO2 is:
= k [NO2]2.
= k [NO]2 [O2].
= k [NO] [O2].
= k [O2].
= k 2[NO2].

The mass-action expression for reversible reaction: N2 (g) + 3H2 (g)  2NH3 (g):
 [N2]2/ [NH3]2
K= [N2]3 [H2].
K= [NH3]2 / [N2] [H2]3
 [H2].
[N2] [H2]3
The mass-action expression for reversible reaction: 3O2 (g) + 2H2S (g)  2H2O (g) + 2SO2 (g):
= [O2]3/ [H3O]2
 [H2S] [O2]3.
K= [SO2]2 / [O2] [H2S]
K= [O2] /[H2O]+ [SO2]
K= [SO2]2[H2O]2 / [O2]3[H2S]2
Rate law equation for reaction: 2 NH3 N2 (g) + 3H2 (g) is:
= k [N2] [H2]3
= k [N]2 [H2].
= k [NH2]3
= k [O2].
= k [N2]2.
The processes in which both catalyst and reagents are in same phase is called:
Heterogeneous catalysis;
Homogeneous catalysis;
Positive catalysis;
Negative catalysis;
Autocatalysis.
Matters, which increase activity of catalyst named:
Promoter (activator)
Inhibitors
Hormones
Indicators
Enzyme
Reactions which are flowing past in two parties: the forward reaction - conducts to formation reaction
product and reverse reaction - decomposing reaction product on mother substances:
Series reaction.
B.
C.
D.
E. *
57.
A.
B. *
Parallel reaction.
Conjugating reaction.
Chain reaction.
Reversible reaction.
Reaction, in which products of firs step reaction is reagents for second step reaction is:
Reversible reaction.
Series reaction.
C.
D.
E.
58.
A. *
B.
C.
Parallel reaction.
Conjugating reaction.
Chain reaction.
Reversible reaction is:
А+В ↔ С+D
В. А→ В→ С→ D
D.
E.
59.
A.
B.
C.
D.
E. *
60.
A.
B.
C. *
D.
E.
61.
A.
B.
C.
D. *
E.
;
А+В→ М; А+С→N
AВ+О· → АО·+В; СD+AO·→CO·+AD
Chain reaction is:
А+В ↔ С+D
А→ В→ С→ D
;
А+В→ М; А+С→N
AВ+О· → АО·+В; СD+AO·→CO·+AD
Parallel reaction is:
А+В ↔ С+D
А→ В→ С→ D
;
А+В→ М; А+С→N
AВ+О· → АО·+В; СD+AO·→CO·+AD
Conjugating reaction is:
;
А+В ↔ С+D
А→ В→ С→ D
А+В→ М; А+С→N
AВ+О· → АО·+В; СD+AO·→CO·+AD
62.
A.
B. *
C.
D.
Series reaction is:
А+В ↔ С+D
А→ В→ С→ D
А+В→ М; А+С→N
AВ+О· → АО·+В; СD+AO·→CO·+AD
E.
63.
A. *
B.
C.
D.
E.
64.
A.
B.
C. *
D.
E.
65.
A.
B.
C.
D. *
E.
66.
A.
B. *
C.
D.
E.
67.
A.
B.
C. *
D.
E.
The process in which liquid reagents react with surface of solid catalyst is named:
Heterogeneous catalysis;
Homogeneous catalysis;
Positive catalysis;
Negative catalysis;
Autocatalysis.
The catalysis in which rate of reaction increase is named:
Heterogeneous catalysis;
Homogeneous catalysis;
Positive catalysis;
Negative catalysis;
Autocatalysis.
The catalysis in which rate of reaction decrease is named:
Heterogeneous catalysis;
Homogeneous catalysis;
Positive catalysis;
Negative catalysis;
Autocatalysis.
The matters which inactive of catalyst named:
Promoters
Inhibitor
Hormone
Indicator
Enzyme.
The nature of enzyme is:
Carbohydrate.
Lipid
Protein.
Mineral acid
Vitamin.
68.
A.
B. *
Proteins specialized to catalyze biological reactions are:
Polymers.
Enzymes.
C.
Hormones.
D.
Indicators.
E.
Vitamin.
69.
A.
B.
C. *
D.
E.
70.
A.
B.
C.
D. *
A substance which can change the speed of а chemical reaction without being used up in that reaction
and the phenomenon is known as:
Polymers.
Hormones.
Catalysts.
Indicators
Vitamin.
Catalyst influence for:
Ganged of chemical equilibrium.
Increase temperature.
Increase pressure;
Rate of reaction.
E.
Increase volume.
71.
A. *
B.
C.
D.
E.
72.
A.
E.
73.
A.
B.
C.
D.
E. *
It is used as catalyst for hydrolysis starch such compound:
HCl.
NaOH.
CuSO4.
CaCl2.
I2.
The reaction of hydrolysis starch is:
C12H22O11 + H2O  2C6H12O6;
nCO2 + mH2O  Cn(H2O)m + nO2;
(C6H10O5)n + nH2O  nC6H12O6;
CH3COOC2H5 + H2O  CH3COOH + C2H5OH.
С6Н12О6 + 6О2→ 6СО2+6Н2О
Biological catalysts are:
Polymers.
Vitamin.
Hormones.
Indicators.
Enzymes.
74.
A.
B. *
C.
D.
E.
Hydrogen electrode is:
Metal-metal ion electrode
Gas-ion electrodes
Metal-insoluble salt-anion electrode
Inert "oxidation-reduction" electrode
Membrane electrode
B.
C. *
D.
75.
E in Nernst equation:
A.
E  E0 -
Mass-action expression
RT
lnQ
nF
is:
B. *
C.
D.
E.
76.
A. *
B.
Electrode potential
Standard electrode potential
EMF
Oxidation potential
Silver electrode is:
Metal-metal ion electrode
Membrane electrode
C.
D.
Gas-ion electrodes
Metal-insoluble salt-anion electrode
E.
Inert "oxidation-reduction" electrode
77.
A.
B.
C. *
D.
E.
The mass-action expression for oxidation-reduction reaction: Fe + CuSO4 = Cu+ FeSO4 is:
Q= 1 / [CuSO4]
Q= [Fe] / [FeSO4] [Cu]
Q= [Cu][FeSO4] / [CuSO4] [Fe]
Q= [Cu] / [CuSO4]
Q= [Fe] /[FeSO4]
78.
E  E0 -
RT
lnQ
nF
is:
A.
B.
C. *
D.
E.
79.
A. *
B.
C.
D.
E.
E0 in Nernst equation:
Mass-action expression
Electrode potential
Standard electrode potential
EMF
Oxidation potential
The mass-action expression for half reaction: Zn2+ + 2e- = Zn is:
Q= [Zn] / [Zn2+]
Q= [Zn2+]2 / [Zn]
Q= [Zn2+] / [Zn]
Q= Zn2+ /Zn
Q= 1 / [Zn2+]2
80.
A.
B.
C.
D.
E. *
Glass electrode is:
Metal-metal ion electrode;
Gas-ion electrodes;
Metal-insoluble salt-anion electrode;
Inert "oxidation-reduction" electrode;
Membrane electrode.
81.
A.
B.
C. *
What value of standard electrode potential for standard hydrogen electrode:
- 0.34;
- 1.22;
0;
D.
+ 0.15;
E.
+ 0.220.
82.
A. *
The mass-action expression for oxidation-reduction reaction 2H+ + 2e- = H2 is:
Q= [H2] / [H+]2
B.
C.
D.
E.
Q= pH2 / [H+]
Q= pH2 / [H+]2
Q= [H+] / pH2
Q= [H+]2 / pH2
83.
A. *
B.
C.
D.
E.
What equation is using for calculated рН solutions in electrochemistry:
Nernst;
Arrhenius;
Electro-neutrality;
Raoult’s;
Shredyngare.
84.
A.
B.
Diagram of silver-silver chloride electrode is:
Pt, H2/2H+.
Ме/Меn+.
C.
D. *
E.
85.
A. *
Zn/Zn2+.
Ag/AgCl, KCl.
Hg/Hg2Cl2, KCl.
Potentiometry is:
Physic-chemical method of research concentration of ions, electrode potential, which used the EMF
measuring;
Aggregation of the particles arising from the stabilizing effect of this secondary minimum;
Increase of the boiling temperature of solutions;
Decline of the freezing temperature of solutions;
System, in which a dispersion phase and dispersion medium are liquids, which are non dissolved eth
other.
Standard hydrogen electrode this:
Platinum lamina is in contact with hydrochloric acid solution.
Platinum lamina is in contact with zinc sulfate solution.
Platinum lamina is in contact with its ions in solution.
Hydrogen at atmospheric pressure is passed into 1 М НС1 in which foil of the platinized platinum
remains immersed through which inflow or outflow of electrons takes place.
A metal is in contact with one of its insoluble salts and also with а solution containing the anion of
the salt
B.
C.
D.
E.
86.
A.
B.
C.
D. *
E.
87.
A. *
B.
C.
What is value of osmotic presure of blood serum?
7,7 -7,8 atm;
6,2 - 7,3 atm;
8,6-8,9 atm;
D.
E.
89.
A.
B. *
C.
2,1 -7,1atm;
10,7-11,4 atm.
Standard EMF of the cell equalled:
pH;
Oxidation number;
Standard oxidation potential of the oxidation half reaction + Standard reduction potential of the
reduction half reaction;
Solubility product;
Heat effect.
What formula is Nernst equation?
E = E0catode - E0anode;
E = E0 - (RT/ nF) ln ([M]/ [Mn+]);
pH = - log [H+];
D.
pH = 14- pOH.
E.
90.
A.
B.
E = 14 - RT/nF
The metal - metal ion electrode is electrode, which:
Employs а gas in contact with its anion or cation in solution.
A metal is in contact with one of its insoluble salts and also with а solution containing the anion of
the salt.
Really no more of an oxidation-reduction electrode than any other.
Semipermeable membrane.
Consists of а metal in contact with its ions in solution.
The gas-ion electrode is electrode, which:
Employs а gas in contact with its anion or cation in solution.
A metal is in contact with one of its insoluble salts and also with а solution containing the anion of
the salt.
Really no more of an oxidation-reduction electrode than any other.
Semipermeation membrane
Consists of а metal in contact with its ions in solution.
In the metal-insoluble salt-anion electrode is electrode, which:
Employs а gas in contact with its anion or cation in solution.
A metal is in contact with one of its insoluble salts and also with а solution containing the anion of
the salt.
Really no more of an oxidation-reduction electrode than any other.
Semipermeation membrane
Consists of а metal in contact with its ions in solution.
An inert oxidation-reduction electrode is:
Employs а gas in contact with its anion or cation in solution.
A metal is in contact with one of its insoluble salts and also with а solution containing the anion of
the salt.
It consists of strip, wire, or of an inert material, say, platinium, in contact with a solution, which
contains ions of a substance, is two different oxidation states.
Semipermeation membrane.
Consists of а metal in contact with its ions in solution.
The difference between the electrode potentials of the two half cell is known as:
D.
E.
88.
A.
B.
C. *
C.
D.
E. *
91.
A. *
B.
C.
D.
E.
92.
A.
B. *
C.
D.
E.
93.
A.
B.
C. *
D.
E.
94.
A. *
B.
C.
D.
E.
95.
A.
B. *
C.
D.
E.
96.
A. *
Electromotive force (EMF) of the cell or cell potential or cell voltage;
Masse-action;
Mole mass;
Molarity;
Solubility product.
Processes, which are between interfaces of two systems is:
Coagulation;
Surface phenomena;
Surface tension;
Absorption;
Boiling.
The equation, which is used for calculate surface tension is:
σ = G/S;
B.
C.
D.
E.
97.
A.
B.
C.
D.
E. *
98.
A.
B.
C.
D.
σ = GS;
σ = S/G;
σ = νRT;
σ = C/RT.
The surfactants are compound, except:
Alcohols;
Alkalis;
Salts of fat acids;
Protein;
Hidrochloric acid..
Energy, which have molecules on surface is:
Enthalpy.
Entropy.
Heat.
Work.
E. *
Free Gibbs’s energy.
99.
A. *
The force in dynes acting upon a line cm long on the surface of the liquid is:
Surface tension.
B.
C.
D.
E.
100.
A.
B.
C.
D. *
E.
Entropy.
Enthalpy.
Heat.
Pressure.
Value of surface free Gibb's energy depends on:
Decrease of pressure.
Volume of liquids.
Form of glass.
Nature of matter.
Freezing temperature.
101.
What concept is correct?
A.
B.
C.
D. *
E.
102.
A.
B.
C.
D. *
E.
103.
A.
B.
C. *
D.
E.
104.
A. *
B.
C.
D.
E.
105.
A.
Surfactant increase surface tension at twice.
Surfactant does not influece on surface tension value.
Surfactant increase surface tension at 4 times.
Surfactant decrease surface tension.
Surfactant increase surface tension in 3 times.
The surfactant is:
Hydrochloric acid.
Calcium hydroxide.
Sodium chloride.
Isoamil alcohol.
Potassium.
The surfactant is all compounds except:
Alcohols.
Fatty acids.
Sodium chloride.
Amino acids.
Proteins.
Surface tension is measured by such unit:
J/m2
N/m2
J/m
J/sm
N/dm2
Surface tension is measured by such unit:
J/sm
B. *
C.
N/m
J/m
D.
E.
106.
N/sm2
N/dm2
What method is used for determination surface tension:
A.
B.
C. *
D.
E.
107.
A.
Potentiometry.
Chelatometry.
Stalagmometric method.
Chromatography.
Criometry.
The concentrated one component in the surface other is named:
Absorption.
B. *
Adsorption.
C.
D.
Disorbsion.
Solubility.
E.
108.
A.
B.
C.
D. *
E.
109.
A. *
Capillary condensation.
What concept is correct?
Surfactant increase surface tension at twice.
Surfactant does not change surface tension.
Surfactant increase surface tension at 4 times.
Surface inactive compound increase surface tension.
Surfactant increase surface tension in 3 times.
Adsorption is:
The phenomenon of concentrated the molecules of а substance on the surface of а liquid or а solid
resulting;
B.
C.
D.
E.
110.
A.
B.
C. *
Chemical reaction between adsorbed and adsorbate;
When molecules have hydrophilic and hydrophobic groups simultaneously;
The separation of mixtures;
The chromatography analysis.
Ionic adsorption this:
The separation of mixtures;
When molecules have hydrophilic and hydrophobic groups simultaneously;
Chemical reaction between solution ions and ions of adsorbent surface;
D.
The chromatography analysis.
E.
111.
A.
B. *
Chemical reaction between adsorbed and adsorbate;
Adsorption of ions is interaction:
Between water and acid;
Between adsorbent ions and ions of solution;
C.
D.
E.
Between liquids;
Between elements;
Between bases.
112.
At chemical adsorption:
A.
B.
C. *
D.
E.
113.
A.
B.
C. *
D.
Is formation intramolecule forces between an adsorbed and an adsorbate;
The concentrated one matter in the volume of other;
Chemical interaction of adsorbent and adsorbate, products to this reaction are in same phase.
There is selective absorption of ones kind of electrolyte ions in surface of ion-exchanger;
The separation of compound in mixture at the thin layer of adsorbed.
The rules of selective adsorption are:
Shulce - Hardy;
Duklo - Trauber;
Pescov-Panet-Faiences';
Vant - Goff;
E.
114.
Raoult’s.
By the rule of selective adsorption an adsorbent must by:
A.
B. *
To be easily soluble compound;
To have a certain crystalline grate;
C.
D.
E.
To be liquid;
To be gaseous;
To be soluble compound.
115.
A. *
B.
C.
D.
The phenomenon of attracting and retaining the molecules of а substance on the surface of а liquid or
а solid resulting into a higher concentration of the molecules on the surface is:
Adsorption
Adsorbate
Adsorbent
Desorption
E.
116.
Absorption
The substance thus adsorbed on the surface is called:
A.
B. *
C.
D.
E.
117.
A.
B.
C. *
Adsorption
Adsorbate
Adsorbent
Desorption
Absorption
The substance on which compound is adsorbed is called:
Adsorption
Adsorbate
Adsorbent
D.
Desorption
E.
118.
A.
B.
C.
D. *
E.
119.
A. *
Absorption
The reverse processes removal of the adsorbed substance from the surface is called:
Adsorption
Adsorbate
Adsorbent
Desorption
Absorption
Adsorbate this:
The substance thus adsorbed on the surface.
B.
C.
D.
The substance on which compound is adsorbed.
Product of reactions.
Reagents of reaction.
E.
120.
A.
Matter which is absorbed
Adsorbent this:
The substance thus adsorbed on the surface.
B. *
The substance on which compound is adsorbed.
C.
D.
E.
121.
Product of reactions.
Reagents of reaction.
Matter which is absorbed
A.
B.
C.
D. *
E.
122.
A. *
B.
C.
D.
E.
123.
A.
B.
К+
Са+2
Fe+3
Sn+4
Na+
Ion exchange adsorption is:
The adsorption in which ions of solution exenge with surface adsorbent ions.
Exchange by electrons
The adsorption in which exchange of molecules.
Absorption of gases by solids.
The adsorption in which of moleculas of solute react with moliculas of solvent.
Cation exchange resins is:
OH--exchange resins
СІ- -exchange resins
C.
D. *
E.
124.
A. *
B.
SO42--exchange resins
H+- exchange resins
Br -- exchange resins
Anion exchange resins is:
OH--exchange resins
Na -exchange resins
C.
D.
E.
125.
A. *
Ca-exchange resins
H+- exchange resins
K-exchange resins
Adsorption is this:
Concentrated one matter in surface other.
B.
C.
D.
E.
126.
A.
B.
C.
D. *
E.
Transferred matters from solid into the gas state.
Method gravimetry.
Method of separation mixtures into individual compounds.
Chromatography analysis.
Chromatography is this:
Concentrated one matter in surface other.
Transferred matters from solid into the gas state.
Method gravimetry.
Method of separation mixtures into individual compounds.
Chelatometry analysis.
What ion has the greatest adsorptive activity?
127.
A.
B.
C. *
D.
E.
128.
A.
B.
C.
D. *
What ion has the greatest adsorptive activity?
E.
129.
A.
B.
C.
D. *
E.
Be+2
130.
A. *
B.
C.
What is particle size of colloid solution?
10-8м;
10-10м;
1015м;
D.
E.
131.
A.
B. *
10-3м;
10-1м
Colloid systems have following properties except:
Sedimentation;
Dinaturation;
C.
D.
E.
Brownian movement effect;
Diffusion;
Osmotic pressure.
132.
A.
B. *
C.
D.
E.
Systems, in which particle size10-4 m are:
True solution;
Macroheterogeneous;
Microheterogeneous;
Ultramicroheterogeneous;
Homogeneous.
133.
A.
B.
C.
D.
What kind of dispersion systems is fog (G-gas, L-Liquid, S-solid)?
G/S;
S/S;
L/L;
G/G;
Sr+2
Са+2
Fe+3
Ba+2
Na+
What ion has the greatest adsorptive activity?
Sr+2
Са+2
Mg+2
Ba+2
Which properties have dispersion systems:
A molecule is structural unit of the system;
Thermodynamics stable system;
Homogeneous system;
Thermodynamics instable system;
The system has not surface between phases.
E. *
134.
A.
B. *
C.
D.
E.
135.
L/G
Method preparation of colloid solutions by this reaction 2Н2S+SO2 = 3S+2H2O is called:
Peptization;.
Oxidation;
Electric method;
Hydrolysis;.
Double decomposition.
Method preparation of colloid solutions by this reaction 2Na2SO4+CaCl = CaSO4+2NaCl is called:
A.
B.
C.
D.
E. *
136.
A.
B.
C.
D. *
E.
Peptization;
Oxidation;
Electric method;
Hydrolysis;
Double decomposition.
Method preparation of colloid solutions by this reaction FeCl3+3H2O= 3HCl + Fe(HO)3 is called:
Peptization;
Oxidation;
Electric method;
Hydrolysis;
Double decomposition.
137.
A. *
B.
C.
D.
E.
138.
A. *
What method is used for separation dispersion particles by sizes?
Electrophoreses;
Brownian motion;
Diffusion;
Sedimentation;
Osmotic pressure
A process of passing of a precipitate into colloidal particles on adding suitable electrolyte is called:
Peptization;
B.
Oxidation;
C.
D.
Electric method;
Hydrolysis;
E.
139.
Double decomposition.
These methods involve the joining together of а large number of smaller particles to form particles of
colloidal size.
Peptization;
A.
B.
C. *
D.
E.
140.
A.
Polymerisation
Condensation;
Titration
Dispersion.
These methods involve the breaking of the bigger particles to colloidal size.
Peptization;
B.
C.
D.
E. *
141.
A.
B.
C.
D. *
E.
142.
A.
B. *
C.
D.
E.
143.
A.
B.
C. *
D.
E.
144.
A.
B.
C. *
D.
E.
Oxidation;
Condensation;
Hydrolysis;
Dispersion.
Systems with dispersed phase particle size between 10-9 to 10-7m are:
True solution;
Macroheterodisperse solution;
Solid;
Colloidal solutions;
Mixture.
For purification colloidal solution is used such method except:
Dialysis
Titration;
Electrodialysis;
Ultrafiltration.
Ultracentrifugation.
What purification colloidal solution method is base in “Artificial kidney”?
Dialysis;
Electrodialysis;
Hemodialysis
Ultrafiltration
Ultracentrifugation
Coagulation this:
The process of separating the particles of colloids from those of crystalloids by diffusion of the
mixture through а parchment or an animal membrane;
Oxidation of element in colloidal solution;
Aggregation of the particles arising from the stabilizing effect of this secondary minimum;
System, in which a dispersion phase and dispersion medium are liquids, which are non dissolved eth
other;
Part of chemistry, which studies physical and chemical properties of microheterogeneous system and
HMC.
145.
The process which involves the movement of colloidal particles towards one or the other electrode when
placed under the influence of an electric field:
A. *
Electrophoresis;
B.
C.
D.
Electrodialysis;
Hemodialysis.
Ultrafiltration.
E.
146.
Ultracentrifugation.
A.
B.
C.
D. *
Electrophoresis;
Electrodialysis;
Hemodialysis;
Electroosmosis;
A phenomenon in which the molecules of the dispersion medium are allowed to move under the influence of
an electric field whereas colloidal particles are not allowed to move:
E.
147.
A.
B. *
C.
D.
E.
148.
Ultracentrifugation.
In а gravitational field, heavy particles settle towards the foot of а column of solution by the process
called:
Ultracentrifugation;
Sedimentation;
Coagulation;
Flocculation;
Dialysis.
The minimum amount of an electrolyte (millimoles) that must be added to one liter of а colloidal solution so as
to bring about complete coagulation or flocculation is called:
A. *
Coagulation or flocculation value (or threshold) of the electrolyte;
B.
C.
D.
E.
149.
A.
B. *
C.
D.
E.
150.
A.
B.
C.
D.
E. *
151.
A.
B.
C.
D. *
E.
152.
A.
B.
C.
D.
E. *
Oxidation number;
Temperature coefficient;
Dissociation degree;
Degree of adsorptions.
Blood is dispersed system, once of dispersed phase particles are erythrocytes with size 10-4 m. What
type of dispersed system is it?
True solution;
Macroheterogeneous;
Microheterogeneous;
Ultramicroheterogeneous;
Colloidal solution.
Blood serum is dispersed system. What type dispersed system is it?
True solution;
Solid;
Macroheterogeneous;
Microheterogeneous;
Colloidal solution.
What kind of dispersion systems is smoke (G-gas, L-Liquid, S-solid)?
G/S;
S/S;
L/L;
S/G;
G/L
System with size dispersed phase particle equal 10-9 - 10-7 is:
True solution;
Microheterogeneous;
Macroheterogeneous;
Homogeneous;
Colloidal solution.
153.
A. *
Colloidal solutions have some stability. What factors influence for they stability?
Electrokinetic ξ -potential.
B.
C.
Pressure.
Volume of systems.
D.
E.
154.
A.
B.
C. *
D.
E.
155.
A.
B.
C. *
D.
E.
156.
A.
B.
C.
D.
E. *
Catalysts.
Indicators.
Colloidal solutions have some stability. Stability is the greatest when:
Thermodynamics ()-potential same as electrokinetic ξ-potential.
Thermodynamics ()-potential greater then electrokinetic ξ-potential.
Thermodynamics ()-potential lest then electrokinetic ξ-potential.
Both equal zero.
Electrokinetic ξ -potential equal zero.
Silver-silver chloride electrode is:
The metal - metal ion electrode;
The gas-ion electrode is electrode;
Metal-insoluble salt-anion electrode;
Inert "oxidation-reduction" electrode;
Membrane electrode.
Coagulants and anticoagulants are used in medicine and pharmacy. What coagulation (flocculation)
value?
Amount of strong acid.
.Amount of base.
Minimum amount of non electrolytes.
Amount of stabilisator.
The minimum amount of an electrolyte (millimoles) that must be added to one liter of а colloidal
solution so as to bring about complete coagulation or flocculation.
A. *
B.
C.
D.
The amount of an electrolyte which is added to one liter of а colloidal solution so as to bring about
complete flocculation is called:
Flocculation number.
Surface tension.
Heat capacity.
Acidity.
E.
158.
A.
B.
C.
D. *
Ion product.
Osmotic pressure of colloidal solution is:
Very great.
Stable all time.
Equal zero.
Very small.
E.
Chang when change illumination.
159.
A.
B.
C.
D. *
E.
Phenomenon of mat luminescence of colloid solution at passing of light:
Coagulation
Peptization.
Diffraction
Opalescence
Nephelomertry.
160.
What polymer is natural?
157.
A.
B.
C.
D. *
E.
Polyethylene;
Kapron;
Polypropilen;
Starch;
Polyformaldehyde.
161.
A. *
B.
C.
D.
E.
162.
A.
B. *
C.
D.
E.
163.
For swellings influence all factors except:
Time;
Temperature;
Relation between energies of bond in a polymer and solving energy;
Concentrations of polymer
Nature polymer.
The quantitative measure of swelling is:
Change of solution volume.
Swelling degree.
Change the nature of polymer.
Unchanging amount of polymer.
Volume of turgescent polymer.
Value of рН solution in which an proteins is in isoelectric state, name ....
A.
B.
C. *
D.
E.
164.
A.
B.
C. *
D.
E.
165.
A.
B. *
C.
D.
E.
166.
A.
B.
C.
Solubility of protein.
Hydrolysis of protein;
Isoelectric point of protein;
Synthesis of protein.
Flowdown of protein
Hydrogen bonds is typical for such structure of proteins:
Quaternary;
Primary;
Secondary;
Tertiary;
Simple.
On the swelling process influence all factors except:
рН medium.
Catalyst.
Nature of polymer and solvent.
Molecular mass of polymer.
Temperature.
What formula is used for determination swelling degree?
α = N/n;
α = K / C;
α = 1- C / m;
D.
E. *
167.
A. *
α = C m / V;
α = (m - m0)/m0 = mp/m0.
The amount of liquids which is absorbed one unit of polymer is named:
Swelling degree;
B.
C.
D.
E.
168.
A.
B. *
C.
D.
E.
169.
A.
B.
C. *
Hydrolysis degree;
Polymerization degree;
Ionizations degree;
Condensation degree.
High molecular connections (HMC) are compounds with molecular mass of order...
10 - 102 atomic units.
104 - 10б atomic units.
10-1 - 10-2 atomic units.
10 - 103 atomic units.
10-4 - 10-б atomic units.
The high molecular compounds (HMC, polymers) are used in pharmacy and medicine. What
property of colloid solution is typical for polymer solutions?
Thermodynamics stability.
Structural viscidity.
Dispersion of light.
D.
Jeling.
E.
170.
A.
B. *
C.
D.
Swelling.
Linked water:
Water which is in the human body;
Water molecules, which pass to the polymer and form hydrate layers;
Water in food;
Water which is adsorbed polymer after formation hydrate layers;
E.
171.
A.
B.
C.
D. *
E.
172.
Creates the compression of the all system.
“Free water”:
Water molecules, which pass to the polymer and form hydrate layers;
Water in the human body;
Water in food;
Water which is adsorbed polymer after formation hydrate layers;
Creates the compression of the all system.
Inreversible is all reaction except:
N2O4(g)  2 NO2(g);
2KClO3 (s)2 KCl(s) + 3O2(g);
CaCO3 (s)  CaO(s) + CO2(g);
2NaNO3  2 NaNO2 + O2;
2Cu(NO3)2  2 CuO + 4NO2 +O2.
The mass-action expression for reversible reaction: C2H4 (g) + H2(g)  C2H6(g).
K = [C2H4] [H2]/ [C2H6];
K = [C2H6] / [C2H4] [H2];
K = [C2H4] + [H2] - [C2H6];
K = [C2H4] / [C2H6];
K = 1/ [C2H6].
Rate law equation for forward reaction: N2O4(g)  2NO2(g) is:
A. *
B.
C.
D.
E.
173.
A.
B. *
C.
D.
E.
174.
A.
B.
C. *
D.
E.
175.
A.
B. *
C.
D.
E.
176.
A. *
B.
C.
D.
E.
177.
A. *
B.
C.
D.
E.
178.
A.
B. *
C.
D.
E.
179.
A.
B.
C. *
D.
E.
180.
A.
B.
C. *
D.
E.
181.
A.
B.
= k [2NO2];
= k [NO2]2;
= k [N2O4];
= k [NO];
= [NO2].
Rate law equation for reverse reaction:
= k [KClO3]2;
= k [KCl]2 [O2]3;
= k 2 [KCl] 3[O2];
= k [KCl] [O2];
= k [KCl] + [O2]3.
Cu/Cu2+ electrode is:
The metal - metal ion electrode;
The gas-ion electrode is electrode;
Metal-insoluble salt-anion electrode;
Inert "oxidation-reduction" electrode;
Membrane electrode.
Zn/Zn2+ electrode is:
The metal - metal ion electrode;
The gas-ion electrode is electrode;
Metal-insoluble salt-anion electrode;
Inert "oxidation-reduction" electrode;
Membrane electrode.
In the metal-insoluble salt-anion electrode is electrode:
Zn/Zn2+ electrode;
Silver-silver chloride electrode;
Hydrogen electrode;
Glass electrode;
Cu/Cu2+ electrode.
Gas-ion electrode is electrode:
Silver-silver chloride electrode;
Zn/Zn2+ electrode;
Hydrogen electrode;
Glass electrode;
Cu/Cu2+ electrode.
Membrane electrode is electrode:
Silver-silver chloride electrode;
Zn/Zn2+ electrode;
Glass electrode;
Hydrogen electrode;
Cu/Cu2+ electrode.
The metal - metal ion electrode is:
Silver-silver chloride electrode;
Calomel electrode;
is:
C.
D.
E. *
182.
A.
B.
C. *
D.
E.
183.
A.
B.
C. *
D.
E.
184.
A.
B. *
C.
D.
E.
185.
A.
B.
C.
D.
E. *
186.
A.
B. *
C.
D.
E.
187.
A. *
B.
C.
D.
E.
188.
A.
Hydrogen electrode;
Glass electrode;
Cd/Cd2+ electrode.
Calomel electrode is:
The metal - metal ion electrode;
The gas-ion electrode is electrode;
Metal-insoluble salt-anion electrode;
Inert "oxidation-reduction" electrode;
Membrane electrode.
For measuring pH of solution and biological liquids is used such electrode:
Zn/Zn2+ electrode;
Calomel electrode;
Hydrogen electrode;
Ag/Ag+ electrode;
Cu/Cu2+ electrode.
For measuring pH of solution and biological liquids is used such electrode:
Calomel electrode;
Glass electrode;
Calomel electrode;
Ag/Ag+ electrode;
Cu/Cu2+ electrode.
If in the half cell, the metal rod is suspended in а solution of one molar concentration, and the
temperature is kept at 298 К, the electrode potential is called:
Membrane potential;
Diffuse potential;
Electro-kinetic potential.
Concentration potential;
Standard electrode potential;
Galvanic cell:
Membrane potential;
pH;
Standard electrode potential;
Concentration potential;
Electro-kinetic potential.
An electrochemical cell:
is used for measuring:
It is а device, which makes use of an oxidation-reduction reaction to produce the interconversion of chemical
and electric energy;
It is а device, which makes use of reaction to produce the interconversion of heat and potential
energy;
It is а device, which makes use of reaction to produce the interconversion of electric and potential
energy;
It is а device, which makes use of reaction to produce the interconversion of chemical and potential
energy;
It is а device, which makes use of a precipitation reaction to produce the interconversion of chemical
and kinetic energy.
Electrode potential is formed in systems when are such reactions:
Double decomposing reaction;
B.
C.
D. *
E.
189.
A. *
B.
C.
D.
E.
190.
A. *
B.
C.
D.
E.
191.
A.
B. *
C.
D.
E.
192.
A.
B.
C. *
D.
E.
193.
A.
B.
C.
D. *
E.
194.
A.
B.
C.
D.
E. *
195.
A.
Hydrolysis reaction;
Precipitation reaction;
Oxidation - redaction reaction:
Neutralization reaction.
This concept “A state of dynamic balance in which the rate of forward and reverse reaction are
equal” is:
Chemical equilibrium;
Constant of reaction rate;
van’t Hoff law;
First law of thermodynamics;
Hass’s law.
The part of the universe chosen for thermodynamic consideration (to study the effect of temperature,
pressure etc.) is called:
System.
Surroundings.
Entropy.
Reaction.
Energy.
The remaining portion of the universe, excluding the system, is called:
System.
Surroundings.
Entropy.
Reaction.
Energy.
The properties of the system whose value depends upon the amount of substance present in the
system are:
Reversible properties.
Irreversible properties.
Extensive properties.
Intensive properties.
Spontaneous properties.
The properties of the system whose value does not depend upon the amount of substance present in
the system are.
Reversible properties.
Irreversible properties.
Extensive properties.
Intensive properties.
Spontaneous properties.
Extensive property is:
Temperature.
Pressure.
Viscosity.
Density.
Mass.
Intensive properties are all except:
Temperature.
B. *
C.
D.
E.
196.
A.
B.
C.
D. *
E.
197.
A.
B.
C. *
D.
E.
198.
A. *
B.
C.
D.
E.
199.
A.
B.
C. *
D.
E.
200.
A.
B.
C. *
D.
E.
201.
A.
B.
Heat capacity.
Viscosity.
Density.
Pressure.
Extensive properties are all except:
Mass.
Volume.
Heat capacity.
Density.
Gibbs free energy.
Intensive property is:
Mass.
Volume.
Viscosity.
Heat capacity.
Gibbs free energy.
Isothermal process is:
А process is carried out in such а manner that the temperature remains constant throughout the
process.
A process is carried out in such а manner that no heat can flow from the system to the surroundings
or vice versa i.e. the system is completely insulated from the surroundings.
А process during which the volume of the system is kept constant.
А process during which the pressure of the system is kept constant.
А process which is carried out infinitesimally slowly so that all changes occurring in the direct
process can be exactly reversed.
Adiabatic process is:
А process during which the volume of the system is kept constant.
А process is carried out in such а manner that the temperature remains constant throughout the
process.
A process is carried out in such а manner that no heat can flow from the system to the surroundings
or vice versa i.e. the system is completely insulated from the surroundings.
А process during which the pressure of the system is kept constant.
А process which is carried out infinitesimally slowly so that all changes occurring in the direct
process can be exactly reversed.
Isochoric process is:
A. А process is carried out in such а manner that the temperature remains constant throughout the
process.
A process is carried out in such а manner that no heat can flow from the system to the surroundings
or vice versa i.e. the system is completely insulated from the surroundings.
А process during which the volume of the system is kept constant.
А process during which the pressure of the system is kept constant.
А process which is carried out infinitesimally slowly so that all changes occurring in the direct
process can be exactly reversed.
Isobaric process is:
А process during which the volume of the system is kept constant.
А process is carried out in such а manner that the temperature remains constant throughout the
process.
C.
D. *
E.
202.
A.
B.
C.
D.
E. *
203.
A. *
B.
C.
D.
E.
204.
A.
B.
C.
D.
E. *
205.
A. *
B.
C.
D.
E.
206.
A.
B.
C.
D. *
E.
207.
A.
B. *
A process is carried out in such а manner that no heat can flow from the system to the surroundings
or vice versa i.e. the system is completely insulated from the surroundings.
А process during which the pressure of the system is kept constant.
А process which is carried out infinitesimally slowly so that all changes occurring in the direct
process can be exactly reversed.
Reversible process is:
А process is carried out in such а manner that the temperature remains constant throughout the
process.
A process is carried out in such а manner that no heat can flow from the system to the surroundings
or vice versa i.e. the system is completely insulated from the surroundings.
А process during which the volume of the system is kept constant.
А process during which the pressure of the system is kept constant.
А process which is carried out infinitesimally slowly so that all changes occurring in the direct
process can be exactly reversed.
Irreversible process is:
A process which does not meet the above requirements.
А process is carried out in such а manner that the temperature remains constant throughout the
process.
А process during which the volume of the system is kept constant.
А process during which the pressure of the system is kept constant.
А process which is carried out infinitesimally slowly so that all changes occurring in the direct
process can be exactly reversed.
For measurement heat is used:
Thermometer.
pH-meter.
Voltmeter.
Potentiometer.
Calorimeter.
The rate of chemical reaction is:
The change in the concentration of any one of the reactants or products per unit of time.
The change in the temperature of any one of the reactants or products per unit of time.
The change in the pressure of solution any one of the reactants or products per unit of time.
The change in the volume of solution any one of the reactants or products per unit of time.
The change in the internal energy of any one of the reactants or products per unit of time.
The rate of chemical reaction is calculated by formula:
W=nRT (V2/V1).
W= pQ.
W=nRTln(V2/V1).
W = p ΔV.
Vant-Goff rule equation is:
W= nRT (V2/V1).
t2/t1 =  t2 - t1/10.
C.
.
D.
E.
208.
A.
B.
C. *
D.
E.
209.
A.
B. *
.
.
W= nRTln(V2/V1).
Factors affection the reaction rate all except:
Nature of the reactants.
Concentration of the reactants.
Internal energy of systems.
Presence of Catalyst.
Surface area of the reactants.
Arhenius equation is:
A. W= nRT (V2/V1).
.
C.
D.
E.
t2/t1 = 
.
W= nRTln(V2/V1).
t2 - t1/10
.
210.
A.
B. *
C.
D.
E.
211.
A. *
B.
C.
D.
E.
212.
A.
B.
C.
D.
E. *
213.
A.
B.
C.
D. *
E.
214.
A.
“A” in Arhenius equation (
) is:
Activation energy.
Pre-exponential factor or the frequency factor.
Boltzmann distribution.
Activation Gibbs energy.
Rate constant.
“Ea” in Arhenius equation (
) is:
Activation energy.
Pre-exponential factor or the frequency factor.
Boltzmann distribution.
Activation Gibbs energy.
Rate constant.
“k” in Arhenius equation (
) is:
Activation energy.
Pre-exponential factor or the frequency factor.
Boltzmann distribution.
Activation Gibbs energy.
Rate constant.
“T” in Arhenius equation (ln k=ln A-Ea/ RT) is:
Activation energy.
Pre-exponential factor or the frequency factor.
Boltzmann distribution.
Temperature.
Rate constant.
Enzyme is biological catalyst. What is it nature?
Carbohydrate.
B.
C. *
D.
E.
215.
A.
B.
C.
D. *
E.
216.
A.
B. *
C.
D.
E.
217.
A.
B.
C.
D.
E. *
218.
A. *
B.
C.
D.
E.
219.
A.
B.
C. *
D.
E.
220.
A.
B.
C.
D. *
E.
221.
A.
B.
C.
D. *
Lipid.
Protein.
Mineral acid.
Vitamin.
HCl is used as catalyst. What is it nature?
Carbohydrate.
Lipid.
Protein.
Mineral acid.
Vitamin.
Platinum is used as catalyst. What is it nature?
Carbohydrate.
Metal.
Protein.
Mineral acid.
Vitamin.
Aluminum cloride is used as catalyst. What is it nature?
Carbohydrate.
Metal.
Protein.
Mineral acid.
Mineral salt.
Cytochrome is biological catalyst. What is it nature?
Protein.
Metal.
Carbohydrate.
Mineral acid.
Mineral salt.
What kind of dispersion systems is emulsions(G-gas, L-Liquid, S-solid)?
G/S.
S/S.
L/L.
S/G.
G/L.
What kind of dispersion systems is gels (G-gas, L-Liquid, S-solid)?
G/S.
S/S.
L/L.
S/L.
G/L.
Syspension is dispersed system with size dispersed phase particle equal 10-4. What type system of it
is(G-gas, L-Liquid, S-solid)?
G/S.
S/S.
L/L.
S/L.
E.
222.
A.
B.
C. *
D.
E.
223.
A. *
B.
C.
D.
E.
224.
A.
B.
C.
D.
E. *
225.
A.
B. *
C.
D.
E.
226.
A.
B.
C.
D.
E. *
227.
A.
B.
C. *
D.
E.
228.
A. *
B.
C.
D.
G/L.
What type of dispersed system is blood if size of dispersed phase particle equal 10-4?
Emulsion.
True solution.
Suspension.
Aerosol.
Colloidal solution.
Aggregation of the particles arising from the stabilizing effect of this secondary minimum is:
Coagulation.
Peptization.
Opalescence.
Diffraction.
Nephelomertry.
Sedimentation is process in which ….
The process of separating the particles of colloids from those of crystalloids by diffusion of the
mixture through а parchment or an animal membrane.
Oxidation of element in colloidal solution.
Aggregation of the particles arising from the stabilizing effect of this secondary minimum.
System, in which a dispersion phase and dispersion medium are liquids, which are non dissolved eth
other.
In а gravitational field, heavy particles settle towards the foot of а column of solution.
These methods involve the joining together of а large number of smaller particles to form particles of
colloidal size is called condensation. What method is condensation?
Nephelomertry.
Peptization.
Oxidation reaction.
Opalescence.
Diffraction.
These condensation methods is all except:
Redaction.
Oxidation.
Double decomposition.
Hydrolysis.
Dispersion.
Oxidation reaction is used for preparation colloidal solution. What reaction is oxidation?
As2O3 + ЗH2S = As2S3 + ЗH2O.
2 AuCl3 + 3 SnCl2=2 Аu + 3SnCl4.
Br2 + H2S = S + 2HBr.
FeCl3 + 3 H2O = Fe(OH)3 + 3 HCl.
AlCl3 + 3 H2O = Al(OH)3 + 3 HCl.
Double decomposition reaction is used for preparation colloidal solution. What reaction is double
decomposition?
As2O3 + ЗH2S = As2S3 + ЗH2O.
2 AuCl3 + 3 SnCl2=2 Аu + 3SnCl4.
Br2 + H2S = S + 2HBr.
FeCl3 + 3 H2O = Fe(OH)3 + 3 HCl.
E.
229.
A.
B.
C. *
D.
E.
230.
A.
B.
C.
D.
E. *
231.
A.
B.
C.
D.
E. *
232.
A.
B. *
C.
D.
E.
233.
A.
B.
C.
D.
E. *
234.
A.
B.
C.
D. *
E.
235.
A. *
B.
C.
D.
E.
236.
A. *
B.
AlCl3 + 3 H2O = Al(OH)3 + 3 HCl.
Reduction reaction is used for preparation colloidal solution. What reaction is reduction?
BrСl2 + H2SO4 → BaSO4 + 2HСl.
As2O3 + ЗH2S = As2S3 + ЗH2O.
2 AuCl3 + 3 SnCl2=2 Аu + 3SnCl4.
FeCl3 + 3 H2O = Fe(OH)3 + 3 HCl.
AlCl3 + 3 H2O = Al(OH)3 + 3 HCl.
Reaction of hydrolysis is used for preparation colloidal solution. What reaction is hydrolysis?
As2O3 + ЗH2S = As2S3 + ЗH2O.
2 AuCl3 + 3 SnCl2=2 Аu + 3SnCl4.
Br2 + H2S = S + 2HBr.
Fe3O3 + 6 HCl = 2 FeCl3 + 3 H2O.
AlCl3 + 3 H2O = Al(OH)3 + 3 HCl.
Colloidal solutions have different properties. Physical properties is all except:
Heterogeneous character.
Stability.
Filterability.
Visibility.
Tyndall affect.
Colloidal solutions have different properties. Colligative properties is:
Heterogeneous character.
Osmotic pressure.
Filterability.
Visibility.
Tyndall affect.
Colloidal solutions have different properties. Optical properties is:
Heterogeneous character.
Osmotic pressure.
Filterability.
Visibility.
Tyndall affect.
Colloidal solutions have different properties. Mechanical properties is:
Heterogeneous character.
Osmotic pressure.
Filterability.
Brownian movement.
Tyndall affect.
Colloidal solutions have different properties. Electrical properties is:
Electrophoresis.
Osmotic pressure.
Filterability.
Brownian movement.
Tyndall affect.
For synthesis of polymers is used reaction:
Addition polymerization.
Oxidation.
C.
D.
E.
237.
A.
B.
C. *
D.
E.
238.
A.
B.
C.
D. *
E.
239.
A.
B. *
C.
D.
E.
240.
A. *
B.
C.
D.
E.
241.
A.
B.
C. *
D.
E.
242.
A.
B.
C.
D. *
E.
243.
A.
B. *
C.
D.
E.
Peptization.
Hydrolysis.
Dispersion.
Colloidal solutions have different properties. Physical properties is:
Electrophoresis.
Electrodialisis.
Filterability.
Brownian movement.
Tyndall affect.
Addition polymerization is reaction……
Oxidation of element in colloidal solution.
The process of separating the particles of colloids from those of crystalloids by diffusion of the
mixture through а parchment or an animal membrane.
Aggregation of the particles arising from the stabilizing effect of this secondary minimum.
Occurs when unsaturated monomers react to form а polymer.
In а gravitational field, heavy particles settle towards the foot of а column of solution.
Anion exchange resins all except:
OH--exchange resins.
H+- exchange resins.
SO42--exchange resins.
СІ- -exchange resins.
Br -- exchange resins.
Cation exchange resins all except:
OH--exchange resins.
Na+-exchange resins.
Ca2+-exchange resins.
H+- exchange resins.
K+-exchange resins.
The occlusion is called:
Concentrated one matter in surface other.
Transferred matters from solid into the gas state.
The adsorption of gases on the surface of metals.
Method of separation mixtures into individual compounds.
Chromatography analysis.
Surface phenomenon is all except:
Adhesion.
Coatings.
Adsorption.
Sedimentation.
Occlusion.
What phenomenon is surface phenomenon?
Titration.
Adhesion.
Neutralization.
Sedimentation.
Absorption.
244.
A.
B.
C. *
D.
E.
245.
A. *
B.
C.
D.
E.
246.
A.
B. *
C.
D.
E.
247.
A. *
B.
C.
D.
E.
248.
A.
B. *
C.
D.
E.
249.
A.
B.
C.
D.
E. *
250.
A.
B.
C.
D. *
E.
251.
A.
B. *
What compound is surface inactive compound?
Alcohols.
Fatty acids.
Sodium
Amino acids.
Proteins.
What ion is adsorbed on OH-- exchange resins?
SO42-.
Na+.
Ca2+.
H+.
K+.
What ion is adsorbed on H+- exchange resins?
SO42-.
Na+.
S2-.
OH-.
Cl-.
On H+- exchange resins is adsorbed all ions except:
PO43-.
Na+.
Ca2+.
H+.
K+.
On OH-- exchange resins is adsorbed all ions except:
SO42-.
Ca2+.
S2-.
OH-.
Cl-.
The adsorption in which ions of solution exchange with surface adsorbent ions.
Adhesion.
Coatings.
Sedimentation.
Occlusion.
Ion exchange adsorption.
Class of compounds, molecule which contain hydrophobic (non-polar) hydrocarbon "tails" and a
hydrophilic (polar) "head" group are called:
Mineral acids.
Mineral Bases.
Oxides.
Surfactants
Mineral salt.
Compounds which concentrate at the interface, and modifies (decrease) its surface tension are called
Mineral acids.
Surfactants.
C.
D.
E.
252.
Mineral Bases.
Oxides.
Mineral salt.
Compounds which accumulates at the interface, and modifies (increase) its surface tension are called:
A.
B.
C.
D. *
E.
253.
A.
B.
C.
D.
E. *
254.
A.
B. *
C.
D.
E.
255.
A.
B.
C.
D. *
E.
256.
A.
B.
C. *
D.
E.
Fatty acids.
Proteins.
Surfactants.
Surface inactive compound.
Phospholipids.
The surface phenomenon on which occurs throughout the body of the material is:
Adhesion.
Adsorption.
Neutralization.
Sedimentation.
Absorption.
The surface phenomenon on which occurs only at the surface of the adsorbent is:
Adhesion.
Adsorption.
Neutralization.
Sedimentation.
Absorption.
Surface tension depend on:
Decrease of pressure.
Volume of liquids.
Form of glass.
Nature of liquids.
Freezing temperature.
The surface tension can determine by such method:
Potentiaometry.
Chelatometry.
Stalagmometry method.
Chromatography.
Criometry.