Download 1. What`s following process that has ∆S0›0? A. All correct B. NH4NO

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What’s following process that has ∆S0›0?
All correct
NH4NO2(s) → 2Н2О(g) + N2(g)
no one
2H2S(g) + 3O2(g) → 2Н2О(g) + 2SO2(g)
2СО(g) + О2(g) →2СО2(g)
Where will the process be spontaneous?
Q=0, ∆S0›0
∆Н0‹0, ∆S0›0
no one
∆Н0›0, Т=0
∆Н0›0, ∆S0‹0
For what is substance the standard enthalpies of formation equal 0?
NO
HF(l)
Н2О(g)
N2(g)
HF(g)
For what is substance the standard enthalpies of formation equal 0?
NO
С6Н12О6
Н2O
СО2
О2
How will the rate of reaction 2 NO(gas) + O2(gas) = 2NO2(gas) change if pressure will increase on 3
times in the system?
increase on 9 times
decrease on 3 times
increase on 3 times
decrease on 27 times
increase on 27 times
How will the rate of this reaction 2 NO(gas) + O2(gas) = 2NO2(gas) change if a pressure will decrease
on 2 times in the system?
decrease on 8 times
decrease on 2 times
increase on 2 times
increase on 6 times
increase on 8 times
The temperature coefficient = 3. How much will the rate of reaction increase at the increasing
temperature on 20 0C?
on 8 times
on 9 times
on 3 times
on 20 times
on 2 times
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How will the rate of this reaction 2 Cl2O = 2 Cl2 + O2 will change if the concentration of Cl2O will
increase on 3 times?
increase on 6 times
decrease on 3 times
increase on 3 times
decrease on 9 times
increase on 9 times
How will a rate of a simple chemical reaction change 2A → B + C at an increasing of initial
concentration on 2 times?
increase on 4
decrease on 4
increase on 2
will not change
decrease on 2
Dependence the rate constant from the temperature is determination according to:
k1 
k0 
1

1

 ln
c0
c
c0  c 
k  Ae
 Ea
RT
1 c0  с

 c0  с
D.
k
E.
1 2 
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For this equation 2Fe(s) + 3Cl2 = 2FeCl3 the rate law is:
1
k  с0
  CCl3
2
B.
  k  C 2Fe  CCl
C.
  k  C Fe  C3Cl
2
D.
  k  C 2Fe  C3Cl
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A.
  k  C3Cl
2
2
2
For this equation С(s) + О2 = СО2 the rate law is:
  CO2  CC
2
B.
2
  k  CO
 CC
2
C.
  k  CO 2  C C
D.
2
  k  CO
2
2
  k  CO
2
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  k  CO 2
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Record of reaction of N2(g)+ O2(g.)= 2NO(g.) - 180,8 kJ/mol means that:
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For formation 2 mol NO is selected 90,4 kJ heat
For formation 1 mol N2 and 1 mol O2 is selected 90,4 kJ heat
For formation1 mol N2 and 1 mol O2 is released 180,8 кJ heat
Under formation of 1 mol of NO 90,4 kJ heat is released
For formation 1 mol of NO is taken of 180,8 kJ heat
To determine, without any calculation, what is the following process that is true of the oxidation
reaction of Glucose: С6H12O6 (l)+ 6O2(g)= CO2(g) + 6H2O(l), H = -2803kJ
Q 0, S 0
H 0, S 0
H 0, S 0
H 0, S 0
H 0, S 0
How much will temperature increase that the rate will increase on 64 times if temperature coefficient
= 2?
40 0C
80 0C
60 0C
50 0C
70 0C
Temperature coefficient shows how much…
The equilibrium constant increases on 10 0C at increasing temperature
The rate’s constant increases on 1 0C at increasing temperature
The rate’s constant increases on 10 0C at increasing temperature
The rate of chemical reaction increases on 1 0C at increasing temperature
The rate of chemical reaction increases after at temperature increas on 10 0 C
From what factors doesn’t depend the rate constant of the chemical reaction?
The nature of reactants
The catalyst presents
The concentrations of reactants
The concentrations of reactants and pressure
Temperature and time
The rate of the chemical reaction is:
All are right
The quantity change of the number of reactants according to the specific time
The concentration change of a reactant according to the specific time
The temperature change of a reactant according to the specific time
The volume change of a reactant according to the specific time
What are the molecularity and the order of a forward reaction 2НІ = Н2+ І2:
Termolecular the first order
Bimolecular the second order
Bimolecular the first order
Unimolecular the second order
Unimolecular the first order
The values of Molecularity and the order as a rule are:
2-3, 2-3 corresponding
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2-3, 1-3 corresponding
0-3, 0-3 corresponding
1-3, 1-3 corresponding
1-3, 0-3 corresponding
For what kind of process using Gibbs’ free energy?
Isobaric
Isochoric
Adiabatic
Isothermic-isochoric
Isothermic-isobaric
What can you define using ΔG?
Chemical rate
Direction of chemistry reaction
Volume
Temperature
Pressure
What kind of properties has the entropy?
Extensive and Intensive
Intensive
A state function
Intensive and state function
Extensive and a state function
What kind of change is indentified the entropy?
Irreversable
No one
Permissible changes & Spontaneous changes
Spontaneous changes
Reversable changes
What is find the entropy change?
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^ S = sum Sproducts = sum Sreactants
ΔS = sum Sproducts – sum Sreactants
ΔS = 1 – (sum Sproducts + sum Sreactants)
E.
Δ S = sum Sreactants + sum Sproducts
Δ S = sum Sreactants – sum Sproducts
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Formula of Entropy are:
S = U+W
S = Q/T
S = U-W
S = T/Q
S = U + dΔV
What is sign of the enthalpy for endothermic process?
-ΔS0
B.
+ΔS0
-ΔH0
0ΔH0
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+ΔH0
How is calculate the enthalpies of reactions?
All correct
ΔH0 = ( Sum of the standard enthalpies of formation of products) : ( Sum of the
standard enthalpies of formation of reactants)
ΔH0 = (Sum of the standard enthalpies of formation of reactants) - ( Sum of the
standard enthalpies of formation of products)
ΔH0 = ( Sum of the standard enthalpies of formation of products) + ( Sum of the
standard enthalpies of formation of reactants)
ΔH0 = ( Sum of the standard enthalpies of formation of products)-( Sum of the standard enthalpies of
formation of reactants)
Record of reaction of N2(g)+ O2(g.)= 2NO(g.) – 180,8 kJ/mol means that:
For formation 2 mol NO is selected 90,4 kJ heat
For formation 1 mol N2 and 1 mol O2 is selected 90,4 kJ heat
For formation1 mol N2 and 1 mol O2 is released 180,8 кJ heat
For formation 1 mol NO is released 90,4 kJ heat
For formation 1 mol of NO is taken of 180,8 kJ heat
What is the law: name energy can neither be created no destroyed although it may be transfered from
one form to another?
Kirkhgof‘s law
Gess’ law
A third law of thermodynamics
A second law of thermodynamics
A first law of thermodynamics
In some systems which are used in pharmaceutical technology volume does not changes. What is
kind of the correlation among internal energy and enthalpy in such systems?
U = 2H
2U = 2H
ΔU > ΔH
ΔU < ΔH
ΔU = ΔH
What is the process according to this reaction of H2(g)+ Cl2(g) → 2HCl(g) + Q= -ΔH:
Intencive
Extensive
Adiabatic
Endothermic
Exothermic
Enthalpy is measured in:
kkal/K
kJ/mol*K
kkal
kJ
kJ/mol
What are the intensive properties of the thermodynamics system:
Initial energy
Concentration
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Internal energy
Volume
Mass
What is the function that doesn’t depend on the passing way of a reaction but depends on the initial
and the final state of a system?
Volume
Pressure
Enthalpy
Work
Heat
Process, when there is V constant is ...
Isothermal
Isochoric
Isobaric
Isochoric– isothermal
Isobaric– isothermal
Open thermodynamic systems are exchanged with an environment:
By nothing
By components
By a matter and energy
By energy
By a matter
How can you classify thermodynamics systems according to their phases?
Irreversible and reversible
equilibrium and unequilibrium
Isolated, opened, closed
Homogeneous and heterogeneous
Solid, liquid, gaseous
Standard condition are when the values of pressure and temperature eqwual:
50 kPа, 298 K
50 kPа, 273 K
101,3 kPа, 298 K
101,3 kPа, 273 K
101,3 kPа, 0 K
When the pressure and the volume are constant. What is name of this thermodynamic process?
Isothermal
Isochoric
Isobaric
Isobaric – isochoric
Isochoric– isothermal
Calcium is.... bond:
Metallic
Nonpolar covalent
Polar covalent
Hydrogen
Ionic
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Hydrogen has ionic bond in compound:
C2H2
CH4
CsH
HCl
H2
Oxygen has nonpolar covalent bond in compound:
СО
CaO
K2O
CO2
O2
The greatest electronegativity has element:
Li
Cl
Br
P
Si
All compounds have ionic bond:
H2S, K2S
SO2, H2SO3
NaCl, KCl
Cl2, SO2
HCl, HBr
All compounds have nonpolar covalent bond:
NaCl, H2O, H2S
H2SO4, K2SO4
NaCl, KCl
N2, O2, Br2
HCl, HBr, H2O
All compounds have polar covalent bond:
NaCl, Cl2, H2
H2SO4, K2SO4
NaCl, KCl
Cl2, H2, Br2
HCl, HBr, H2O
What molecule has multiple bonds?
I2
HCl
N2
H2
polar molecule
The most polar is ….bond:
Hydrogen
Metallic
Ionic
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Nonpolar covalent
Polar covalent
Intermolecular hydrogen bond is between molecules of:
F2
K2S
N2
H2
HF
Between water molecules are…. bond
Metallic
Nonpolar covalent
Polar covalent
Hydrogen
Ionic
All compounds have polar covalent bond except:
O3
NH3
HF
H2O
H2SO4
What molecule has nonpolar covalent bond?
NO
H2
HF
H2O
H2SO4
Choose a compound which has nonpolar covalent bond is:
Cu
H2S
F2
H2O
K2O
Choose a compound which has ionic bond is:
Cu
H2S
F2
H2O
K2O
How many periods are in the periodical table of D. Mendeleev?
6
8
7
4
3
The greatest nonmetallic properties has:
S
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Na
Cl
F
Ag
The greatest metallic properties has:
Li
Na
Cl
Fr
F
How many electrons are at f-lever?
8
10
16
6
14
How many electrons are at d-lever?
8
10
16
6
2
How many electrons are at p-lever?
7
32
16
6
2
How many electrons are at s-orbital?
2
32
16
8
3
The smallest unit of a chemical element that has the properties of that element is called:
Atom
Molecule
Nucleon
Electron
Neutron
What is spin?
Type of hybridization
Electronic orbitales
Charge of nucleus of atom
Electronic density
Own motion of electron is about axis
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Two or more atoms having the same atomic number but differing in atomic weight and mass number
is named:
Protons
Isochors
Isotones
Isotopes
Spin
Five electrons on a p electronic level have an atom:
Argon
Neon
Fluorine
Nitrogen
Carbon
The atomic mass is determined as:
Sum mass of all electrons which are in atom
Sum mass of neutrons which are in nucleus
Sum mass of all protons and neutrons which are in nucleus
Sum mass of all electrons which are in main electronic levels
Sum mass of protons which are in nucleus
What particle is influence for charge of atomic nucleus?
Amount of protons
Amount of electrons
Common amount of nucleons
Amount of neutrons
Amount of positrons
What particle is not in the atomic nucleus?
Any one
Proton
Nucleon
Electron
Neutron
Non-salts forming oxides are:
CuO, NaOH, Ba(OH)2, Fe(OH)3, ZnO
CO, N2O, NO, SiO, H2O
SO2; SO3; P2O5; Mn2O7; CrO3
ZnO; Al2O3; Cr2O3; SnO2
Na2O; MgO; CuO
Amphoteric oxides are:
CuO, NaOH, Ba(OH)2, Fe(OH)3, ZnO
CO, N2O, NO, SiO, H2O
SO2; SO3; P2O5; Mn2O7; CrO3
ZnO; Al2O3; Cr2O3; SnO2
Na2O; MgO; CuO
Complex substances are all except:
HCl
Cl2
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Fe(OH)3
MgO
BaCO3
Acidic oxides are:
CuO, NaOH, Ba(OH)2, Fe(OH)3, ZnO
CO, N2O, NO, SiO, H2O
SO2; SO3; P2O5; Mn2O7; CrO3
ZnO; Al2O3; Cr2O3; SnO2
Na2O; MgO; CuO
Basic oxides are:
CuO, NaOH, Ba(OH)2, Fe(OH)3, ZnO
CO, N2O, NO, SiO, H2O
SO2; SO3; P2O5; Mn2O7; CrO3
ZnO; Al2O3; Cr2O3; SnO2
Na2O; MgO; CuO
Salts are:
HCl, HBr, H2S, HNO3, H3PO4
C, Cl2, KOH, CuO, H2SO4, NaH
CuOH, NaOH, Ba(OH)2, Fe(OH)3, Zn (OH)2
MgO, Al2O3, Cr2O3, SO3, P2O5, CrO3
BaCO3, CaCl2, MgCl2, Na3PO4,Ca3(PO4)2
Oxides are:
HCl, HBr, H2S, HNO3, H3PO4
C, Cl2, KOH, CuO, H2SO4, NaH
CuOH, NaOH, Ba(OH)2, Fe(OH)3, Zn (OH)2
MgO, Al2O3, Cr2O3, SO3, P2O5, CrO3
BaCO3. CaCl2, MgCl2, 2Na3PO4,Ca3(PO4)2
Bases are:
HCl, HBr, H2S, HNO3, H3PO4
C, Cl2, KOH, CuO, H2SO4, NaH
CuOH, NaOH, Ba(OH)2, Fe(OH)3, Zn (OH)2
MgO, Al2O3, Cr2O3, SO3, P2O5, CrO3
BaCO3. CaCl2, MgCl2, 2Na3PO4,Ca3(PO4)2
Acids are:
HCl, HBr, H2S, HNO3, H3PO4
C, Cl2, KOH, CuO, H2SO4, NaH
CuOH, NaOH, Ba(OH)2, Fe(OH)3, Zn (OH)2
MgO, Al2O3, Cr2O3, SO3, P2O5, CrO3
BaCO3. CaCl2, MgCl2, 2Na3PO4,Ca3(PO4)2
Complex salts are:
[Ag(NH3)2]Br, Na[Ag(CN)2]
NaHCO3, Na2HPO4
CaOCl2, KAl(SO4)2
Na2SO4, CaCl2
Zn(OH)Cl, Al(OH)2Br
Mixed salts are:
A.
B.
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E.
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KAl(SO4)2
NaHCO3, Na2HPO4
CaOCl2
Na2SO4, CaCl2
Zn(OH)Cl, Al(OH)2Br
Basic salts are:
KAl(SO4)2
NaHCO3, Na2HPO4
CaOCl2
Na2SO4, CaCl2
Zn(OH)Cl, Al(OH)2Br
Double salts are:
KAl(SO4)2
NaHCO3, Na2HPO4
CaOCl2
Na2SO4, CaCl2
Zn(OH)Cl, Al(OH)2Br
Acidic salts are:
KAl(SO4)2
NaHCO3, Na2HPO4
CaOCl2
Na2SO4, CaCl2
Zn(OH)Cl, Al(OH)2Br
Medium salts are:
KAl(SO4)2
NaHCO3, Na2HPO4
Zn(OH)Cl
Na2SO4, CaCl2
Zn(OH)Cl, Al(OH)2Br
Mixed salts are:
In the time of dissociation gives two cations and one anion
In the time of dissociation give only metal cations, hydroxyl anions and anions of acid radical.
Formed by means of one cation and two anions
In the time of dissociation give only metal cations (or NH4+), hydrogen anions and anions of acid
radical
In the time of dissociation give only metal cations (or NH4+) and ions of acid radical
Basic salts are:
In the time of dissociation gives two cations and one anion
Under the dissociation give metal cations, hydroxyl anions and anions of acid
Formed by means of one cation and two anions
In the time of dissociation give only metal cations (or NH4+), hydrogen anions and anions of acid
In the time of dissociation give only metal cations (or NH4+) and ions of acid
Double salts are:
Two cations and one anion are created during dissociation
In the time of dissociation give only metal cations, hydroxyl anions and anions of acid radical
Formed by means of one cation and two anions
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In the time of dissociation give only metal cations (or NH4+), hydrogen ions and anions of acid
radical
In the time of dissociation give only metal cations (or NH4+) and ions of acid radical
Acidic salts are:
In the time of dissociation gives two cations and one anion
In the time of dissociation give only metal cations, hydroxyl anions and anions of acid radical
Formed by means of one cation and two anions
In the time of dissociation give only metal cations (or NH4+), hydrogen ions and anions of acid
radical
In the time of dissociation give only metal cations (or NH4+ ) and ions of acid radical
Medium salts are:
In the time of dissociation gives two cations and one anion
In the time of dissociation give only metal cations, hydroxyl anions and anions of acid radical
Formed by means of one cation and two anions
In the time of dissociation give only metal cations (or NH4+), hydrogen ions and anions of acid
radical
In the time of dissociation give only metal cations (or NH4+) and anions of acid radical
Salts are:
Complex substances, which consist from atoms of metal and acid residuals
Complex substances, consisting from hydrogen atoms
Complex substances, in which atoms of metals bonded with one or several hydroxyls groups
Complex substances, consisting from two elements, one of which oxygen
Compound which molecules consist of one-type atoms
Acids are:
Complex substances, which consist from atoms of metal and acid residuals. This the most multiple
class of inorganic compounds
Complex substances, consisting of hydrogen cations and anion
Complex substances, in which atoms of metals bonded with one or several hydroxyls groups
Complex substances, consisting from two elements, one of which is oxygen
Compound which molecules consist of one-type atoms
Bases are:
Complex substances, which consist from atoms of metal and acid residuals. This the most multiple
class of inorganic compounds
Complex substances, consisting from hydrogen atoms
Complex substances, in which atoms of metals bonded with one or several hydroxyls groups
Complex substances, consisting from two elements, one of which oxygen
Compound which molecules consist of one-type atoms
Oxides are:
Complex substances, which consist from atoms of metal and acid residuals. This the most multiple
class of inorganic compounds
Complex substances, consisting from hydrogen atoms
Complex substances, in which atoms of metals bonded with one or several hydroxyls groups
Complex substances, consisting from two elements, one of which oxygen
Compound which molecules consist of one-type atoms
Monoatomic compound is:
Water
Helium
C.
D.
E.
95.
A.
B.
C. *
D.
E.
96.
A.
B.
C.
D.
E. *
97.
A.
B.
C.
D. *
E.
98.
A.
B.
C.
D. *
E.
99.
A. *
B.
C.
D.
E.
100.
A. *
B.
C.
D.
E.
101.
A.
B.
C.
D. *
E.
102.
Ozone
Ammonia
Oxygen
Such compound has three atoms in molecule:
Aluminum hydride
Hydrogen fluorine
Hydrogen sulfur
Ammonia
Methanol
Formula of molecule is:
ОН3O
2O
O-2
O2
Molar mass of sulfuric acid is:
49 g/mole
80 g/mole
106 g/mole
98 g/mole
65 g/mole
Mass of three mole of water is:
6g
36 g
48 g
54 g
18 g
Relative atomic mass of carbon is:
12
14
6
10
18
Avogadro’s number is:
6.02*1023
6.02*1025
3.01*1023
6.02*1022
3.01*1020
Molar mass of water is:
18 g
17 g/mole
24 g/mole
18 g/mole
16 g/mole
Relative atomic mass of Oxygen is:
A.
B.
C.
D.
E. *
103.
A.
B. *
C.
D.
E.
104.
A.
B.
C. *
D.
E.
105.
A.
B.
C. *
D.
E.
106.
A.
B.
C.
D.
E. *
107.
A. *
B.
C.
D.
E.
108.
A.
B.
C.
D.
E. *
109.
A.
B.
C. *
D.
8
15
12
18
16
Molar volume at normal stat (a temperature 273 K and pressure of 101,3 kPa) has:
22,4 m3
22,4 l/mol
11,2 l/mole
lest then 22,4 l/mole
more than 22,4 l/mole
During the physical phenomena:
There is a change of quantitative composition of compound
There is a change of amount of electrons in an atom
There is a change of the aggregate state of compound
There is a change only of chemical elements
There is a change of qualitative composition of molecules
112 g of nitrogen have volume:
56,9 l
11,2 l
89,6 l
112 l
22,4 l
Complex compound:
О3
C
О2
H2
СО2
Choose correct definition “simple compound is…..”
molecules or crystals are contain atoms of one element
molecules or crystals are contain atoms of 3th different elements
molecules or crystals are contain atoms of one group elements
molecules or crystals are contain atoms of 2th elements
molecules or crystals are contain atoms of different elements
To choose oxygen-containing acids:
H2S
HBr
HCl
HI
H2SO4
To choose the simple compound:
HNО3
CO
О2
H2O
E.
110.
A.
B.
C.
D. *
E.
111.
A.
B.
C.
D. *
E.
112.
A.
B.
C.
D.
E. *
113.
A.
B.
C.
D.
E. *
114.
A. *
B.
C.
D.
E.
115.
A.
B. *
C.
D.
E.
116.
A.
B.
C.
D.
СО2
What’s following process that has ΔS0›0?
All correct
NH4NO2(s) > 2Н2О(g) + N2(g)
no one
2H2S(g) + 3O2(g) > 2Н2О(g) + 2SO2(g)
2СО(g) + О2(g) >2СО2(g)
For what is substance the standard enthalpies of formation equal 0?
NO
HF(l)
Н2О(g)
N2(g)
HF(g)
For what is substance the standard enthalpies of formation equal 0?
NO
С6Н12О6
Н2O
СО2
О2
How will the rate of reaction 2 NO(gas) + O2(gas) = 2NO2(gas) change if pressure will increase
on 3 times in the system?
increase on 9 times
decrease on 3 times
increase on 3 times
decrease on 27 times
increase on 27 times
How will the rate of this reaction 2 NO(gas) + O2(gas) = 2NO2(gas) change if a pressure will
decrease on 2 times in the system?
decrease on 8 times
decrease on 2 times
increase on 2 times
increase on 6 times
increase on 8 times
The temperature coefficient = 3. How much will the rate of reaction increase at the increasing
temperature on 20 0C?
on 8 times
on 9 times
on 3 times
on 20 times
on 2 times
How will the rate of this reaction 2 Cl2O = 2 Cl2 + O2 will change if the concentration of Cl2O will
increase on 3 times?
increase on 6 times
decrease on 3 times
increase on 3 times
decrease on 9 times
E. *
117.
A. *
B.
C.
D.
E.
118.
A.
B.
C. *
D.
E.
119.
A.
B.
C.
D. *
E.
120.
A.
B.
C. *
D.
E.
121.
A.
B.
C.
D.
E. *
122.
A.
B.
C.
D.
E. *
123.
A.
B.
C. *
D.
E.
124.
increase on 9 times
How will a rate of a simple chemical reaction change 2A > B + C at an increasing of initial
concentration on 2 times?
increase on 4
decrease on 4
increase on 2
will not change
decrease on 2
Dependence the rate constant from the temperature is determination according to:
_
_
_
_
_
Record of reaction of N2(g)+ O2(g.)= 2NO(g.) - 180,8 kJ/mol means that:
For formation 2 mol NO is selected 90,4 kJ heat
For formation 1 mol N2 and 1 mol O2 is selected 90,4 kJ heat
For formation1 mol N2 and 1 mol O2 is released 180,8 кJ heat
Under formation of 1 mol of NO 90,4 kJ heat is released
For formation 1 mol of NO is taken of 180,8 kJ heat
How much will temperature increase that the rate will increase on 64 times if temperature
coefficient = 2?
40 0C
80 0C
60 0C
50 0C
70 0C
Temperature coefficient shows how much…
The equilibrium constant increases on 10 0C at increasing temperature
The rate’s constant increases on 1 0C at increasing temperature
The rate’s constant increases on 10 0C at increasing temperature
The rate of chemical reaction increases on 1 0C at increasing temperature
The rate of chemical reaction increases after at temperature increas on 10 0 C
From what factors doesn’t depend the rate constant of the chemical reaction?
The nature of reactants
The catalyst presents
The concentrations of reactants
The concentrations of reactants and pressure
Temperature and time
The rate of the chemical reaction is:
All are right
The quantity change of the number of reactants according to the specific time
The concentration change of a reactant according to the specific time
The temperature change of a reactant according to the specific time
The volume change of a reactant according to the specific time
What are the molecularity and the order of a forward reaction 2НІ = Н2+ І2:
A.
B. *
C.
D.
E.
125.
A.
B.
C.
D.
E. *
126.
A.
B.
C.
D.
E. *
127.
A.
B. *
C.
D.
E.
128.
A.
B.
C.
D.
E. *
129.
A.
B.
C.
D. *
E.
130.
A.
B. *
C.
D.
E.
131.
A.
B.
Termolecular the first order
Bimolecular the second order
Bimolecular the first order
Unimolecular the second order
Unimolecular the first order
The values of Molecularity and the order as a rule are:
2-3, 2-3 corresponding
2-3, 1-3 corresponding
0-3, 0-3 corresponding
1-3, 1-3 corresponding
1-3, 0-3 corresponding
For what kind of process using Gibbs’ free energy?
Isobaric
Isochoric
Adiabatic
Isothermic-isochoric
Isothermic-isobaric
What can you define using ?G?
Chemical rate
Direction of chemistry reaction
Volume
Temperature
Pressure
What kind of properties has the entropy?
Extensive and Intensive
Intensive
A state function
Intensive and state function
Extensive and a state function
What kind of change is indentified the entropy?
Irreversable
No one
Permissible changes & Spontaneous changes
Spontaneous changes
Reversable changes
Formula of Entropy are:
S = U+W
S = Q/T
S = U-W
S = T/Q
S = U + d?V
How is calculate the enthalpies of reactions?
All correct
?H0 = ( Sum of the standard enthalpies of formation of products) : ( Sum of the standard enthalpies
of formation of reactants)
C.
D.
E. *
132.
A.
B.
C.
D. *
E.
133.
A.
B.
C.
D.
E. *
134.
A.
B.
C.
D.
E. *
135.
A.
B.
C.
D.
E. *
136.
A.
B. *
C.
D.
E. *
137.
A.
B. *
C.
D.
E.
138.
A.
?H0 = (Sum of the standard enthalpies of formation of reactants) - ( Sum of the standard
enthalpies of formation of products)
?H0 = ( Sum of the standard enthalpies of formation of products) + ( Sum of the standard enthalpies
of formation of reactants)
?H0 = ( Sum of the standard enthalpies of formation of products)-( Sum of the standard enthalpies of
formation of reactants)
Record of reaction of N2(g)+ O2(g.)= 2NO(g.) – 180,8 kJ/mol means that:
For formation 2 mol NO is selected 90,4 kJ heat
For formation 1 mol N2 and 1 mol O2 is selected 90,4 kJ heat
For formation1 mol N2 and 1 mol O2 is released 180,8 кJ heat
For formation 1 mol NO is released 90,4 kJ heat
For formation 1 mol of NO is taken of 180,8 kJ heat
What is the law: name energy can neither be created no destroyed although it may be transfered
from one form to another?
Kirkhgof‘s law
Gess’ law
A third law of thermodynamics
A second law of thermodynamics
A first law of thermodynamics
In some systems which are used in pharmaceutical technology volume does not changes. What is
kind of the correlation among internal energy and enthalpy in such systems?
U = 2H
2U = 2H
?U > ?H
?U < ?H
?U = ?H
What is the process according to this reaction of H2(g)+ Cl2(g) > 2HCl(g) + Q= -ΔH:
Intencive
Extensive
Adiabatic
Endothermic
Exothermic
Enthalpy is measured in:
kkal/K
kJ/molK
kkal
kJ
kJ/mol
What are the intensive properties of the thermodynamics system:
Initial energy
Concentration
Internal energy
Volume
Mass
What is the function that doesn’t depend on the passing way of a reaction but depends on the initial
and the final state of a system?
Volume
B.
C. *
D.
E.
139.
A.
B. *
C.
D.
E.
140.
A.
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.
145.
A.
B.
C. *
D.
E.
Pressure
Enthalpy
Work
Heat
Process, when there is V constant is ...
Isothermal
Isochoric
Isobaric
Isochoric– isothermal
Isobaric– isothermal
Open thermodynamic systems are exchanged with an environment:
By nothing
By components
By a matter and energy
By energy
By a matter
How can you classify thermodynamics systems according to their phases?
Irreversible and reversible
equilibrium and unequilibrium
Isolated, opened, closed
Homogeneous and heterogeneous
Solid, liquid, gaseous
Standard condition are when the values of pressure and temperature equal:
50 kPа, 298 K
50 kPа, 273 K
101,3 kPа, 298 K
101,3 kPа, 273 K
101,3 kPа, 0 K
When the pressure and the volume are constant. What is name of this thermodynamic process?
Isothermal
Isochoric
Isobaric
Isobaric – isochoric
Isochoric– isothermal
Calcium has.... bond:
Metallic
Nonpolar covalent
Polar covalent
Hydrogen
Ionic
Hydrogen has ionic bond in compound:
C2H2
CH4
CsH
HCl
H2
146.
A.
B.
C.
D.
E. *
147.
A.
B. *
C.
D.
E.
148.
A.
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.
153.
A.
B.
C.
Oxygen has nonpolar covalent bond in compound:
СО
CaO
K2O
CO2
O2
The greatest electronegativity has element:
Li
Cl
Br
P
Si
All compounds have ionic bond:
H2S, K2S
SO2, H2SO3
NaCl, KCl
Cl2, SO2
HCl, HBr
All compounds have nonpolar covalent bond:
NaCl, H2O, H2S
H2SO4, K2SO4
NaCl, KCl
N2, O2, Br2
HCl, HBr, H2O
All compounds have polar covalent bond:
NaCl, Cl2, H2
H2SO4, K2SO4
NaCl, KCl
Cl2, H2, Br2
HCl, HBr, H2O
What molecule has multiple bonds?
I2
HCl
N2
H2
polar molecule
The most polar is ….bond:
Hydrogen
Metallic
Ionic
Nonpolar covalent
Polar covalent
Intermolecular hydrogen bond is between molecules of:
F2
K2S
N2
D.
E. *
154.
A.
B.
C.
D. *
E.
155.
A. *
B.
C.
D.
E.
156.
A.
B. *
C.
D.
E.
157.
A.
B.
C. *
D.
E.
158.
A.
B.
C.
D.
E. *
159.
A.
B.
C. *
D.
E.
160.
A.
B. *
C.
D.
E.
161.
A.
H2
HF
Between water molecules is…. bond
Metallic
Nonpolar covalent
Polar covalent
Hydrogen
Ionic
All compounds have polar covalent bond except:
O3
NH3
HF
H2O
H2SO4
What molecule has nonpolar covalent bond?
NO
H2
HF
H2O
H2SO4
Choose a compound which has nonpolar covalent bond is:
Cu
H2S
F2
H2O
K2O
Choose a compound which has ionic bond is:
Cu
H2S
F2
H2O
K2O
How many periods are in the periodical table of D. Mendeleev?
6
8
7
4
3
How many are groups in periodical table of D. Mendeleeva?
6
8
9
4
5
The greatest nonmetallic properties has:
S
B.
C.
D. *
E.
162.
A.
B.
C.
D. *
E.
163.
A.
B.
C.
D.
E. *
164.
A.
B. *
C.
D.
E.
165.
A.
B.
C.
D. *
E.
166.
A. *
B.
C.
D.
E.
167.
A. *
B.
C.
D.
E.
168.
A.
B.
C.
D.
E. *
Na
Cl
.F
Ag
The greatest metallic properties has:
Li
Na
Cl
Fr
F
How many electrons are at f-lever?
8
10
16
6
14
How many electrons are at d-lever?
8
10
16
6
2
How many electrons are at p-lever?
7
32
16
6
2
How many electrons are at s-orbital?
2
32
16
8
3
The smallest unit of a chemical element that has the properties of that element is called:
Atom
Molecule
Nucleon
Electron
Neutron
What is spin?
Type of hybridization
Electronic orbitales
Charge of nucleus of atom
Electronic density
Own motion of electron is about axis
169.
A.
B.
C.
D. *
E.
170.
A.
B.
C. *
D.
E.
171.
A.
B.
C. *
D.
E.
172.
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. *
Two or more atoms having the same atomic number but differing in atomic weight and mass
number is named:
Protons
Isochors
Isotones
Isotopes
Spin
Five electrons on a p electronic level have an atom:
Argon
Neon
Fluorine
Nitrogen
Carbon
The atomic mass is determined as:
Sum mass of all electrons which are in atom
Sum mass of neutrons which are in nucleus
Sum mass of all protons and neutrons which are in nucleus
Sum mass of all electrons which are in main electronic levels
Sum mass of protons which are in nucleus
What particle is influence for charge of atomic nucleus?
Amount of protons
Amount of electrons
Common amount of nucleons
Amount of neutrons
Amount of positrons
What particle is not in the atomic nucleus?
Any one
Proton
Nucleon
Electron
Neutron
Non-salts forming oxides are:
CuO, NaOH, Ba(OH)2, Fe(OH)3, ZnO
CO, N2O, NO, SiO, H2O
SO2; SO3; P2O5; Mn2O7; CrO3
ZnO; Al2O3; Cr2O3; SnO2
Na2O; MgO; CuO
Amphoteric oxides are:
CuO, NaOH, Ba(OH)2, Fe(OH)3, ZnO
CO, N2O, NO, SiO, H2O
SO2; SO3; P2O5; Mn2O7; CrO3
ZnO; Al2O3; Cr2O3; SnO2
Na2O; MgO; CuO
Complex substances are all except:
HCl
Cl2
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.
C. *
D.
E.
182.
A. *
B.
C.
D.
E.
183.
A. *
B.
C.
D.
E.
184.
Fe(OH)3
MgO
BaCO3
Acidic oxides are:
CuO, NaOH, Ba(OH)2, Fe(OH)3, ZnO
CO, N2O, NO, SiO, H2O
SO2; SO3; P2O5; Mn2O7; CrO3
ZnO; Al2O3; Cr2O3; SnO2
Na2O; MgO; CuO
Basic oxides are:
CuO, NaOH, Ba(OH)2, Fe(OH)3, ZnO
CO, N2O, NO, SiO, H2O
SO2; SO3; P2O5; Mn2O7; CrO3
ZnO; Al2O3; Cr2O3; SnO2
Na2O; MgO; CuO
Salts are:
HCl, HBr, H2S, HNO3, H3PO4
C, Cl2, KOH, CuO, H2SO4, NaH
CuOH, NaOH, Ba(OH)2, Fe(OH)3, Zn (OH)2
MgO, Al2O3, Cr2O3, SO3, P2O5, CrO3
BaCO3, CaCl2, MgCl2, Na3PO4,Ca3(PO4)2
Oxides are:
HCl, HBr, H2S, HNO3, H3PO4
C, Cl2, KOH, CuO, H2SO4, NaH
CuOH, NaOH, Ba(OH)2, Fe(OH)3, Zn (OH)2
MgO, Al2O3, Cr2O3, SO3, P2O5, CrO3
BaCO3. CaCl2, MgCl2, 2Na3PO4,Ca3(PO4)2
Bases are:
HCl, HBr, H2S, HNO3, H3PO4
C, Cl2, KOH, CuO, H2SO4, NaH
CuOH, NaOH, Ba(OH)2, Fe(OH)3, Zn (OH)2
MgO, Al2O3, Cr2O3, SO3, P2O5, CrO3
BaCO3. CaCl2, MgCl2, 2Na3PO4,Ca3(PO4)2
Acids are:
HCl, HBr, H2S, HNO3, H3PO4
C, Cl2, KOH, CuO, H2SO4, NaH
CuOH, NaOH, Ba(OH)2, Fe(OH)3, Zn (OH)2
MgO, Al2O3, Cr2O3, SO3, P2O5, CrO3
BaCO3. CaCl2, MgCl2, 2Na3PO4,Ca3(PO4)2
Complex salts are:
[Ag(NH3)2]Br, Na[Ag(CN)2]
NaHCO3, Na2HPO4
CaOCl2, KAl(SO4)2
Na2SO4, CaCl2
Zn(OH)Cl, Al(OH)2Br
Mixed salts are:
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.
B.
C.
D. *
E.
189.
A.
B.
C. *
D.
E.
190.
A.
B. *
C.
D.
E.
191.
A. *
B.
C.
KAl(SO4)2
NaHCO3, Na2HPO4
CaOCl2
Na2SO4, CaCl2
Zn(OH)Cl, Al(OH)2Br
Basic salts are:
KAl(SO4)2
NaHCO3, Na2HPO4
CaOCl2
Na2SO4, CaCl2
Zn(OH)Cl, Al(OH)2Br
Double salts are:
KAl(SO4)2
NaHCO3, Na2HPO4
CaOCl2
Na2SO4, CaCl2
Zn(OH)Cl, Al(OH)2Br
Acidic salts are:
KAl(SO4)2
NaHCO3, Na2HPO4
CaOCl2
Na2SO4, CaCl2
Zn(OH)Cl, Al(OH)2Br
Medium salts are:
KAl(SO4)2
NaHCO3, Na2HPO4
Zn(OH)Cl
Na2SO4, CaCl2
Zn(OH)Cl, Al(OH)2Br
Mixed salts are:
In the time of dissociation gives two cations and one anion
In the time of dissociation give only metal cations, hydroxyl anions and anions of acid radical.
Formed by means of one cation and two anions
In the time of dissociation give only metal cations (or NH4+), hydrogen anions and anions of acid
radical
In the time of dissociation give only metal cations (or NH4+) and ions of acid radical
Basic salts are:
In the time of dissociation gives two cations and one anion
Under the dissociation give metal cations, hydroxyl anions and anions of acid
Formed by means of one cation and two anions
In the time of dissociation give only metal cations (or NH4+), hydrogen anions and anions of acid
In the time of dissociation give only metal cations (or NH4+) and ions of acid
Double salts are:
Two cations and one anion are created during dissociation
In the time of dissociation give only metal cations, hydroxyl anions and anions of acid radical
Formed by means of one cation and two anions
D.
E.
192.
A.
B.
C.
D. *
E.
193.
A.
B.
C.
D.
E. *
194.
A. *
B.
C.
D.
E.
195.
A.
B. *
C.
D.
E.
196.
A.
B.
C. *
D.
E.
197.
A.
B.
C.
D. *
E.
198.
A.
B. *
In the time of dissociation give only metal cations (or NH4+), hydrogen ions and anions of acid
radical
In the time of dissociation give only metal cations (or NH4+) and ions of acid radical
Acidic salts are:
In the time of dissociation gives two cations and one anion
In the time of dissociation give only metal cations, hydroxyl anions and anions of acid radical
Formed by means of one cation and two anions
In the time of dissociation give only metal cations (or NH4+), hydrogen ions and anions of acid
radical
In the time of dissociation give only metal cations (or NH4+ ) and ions of acid radical
Medium salts are:
In the time of dissociation gives two cations and one anion
In the time of dissociation give only metal cations, hydroxyl anions and anions of acid radical
Formed by means of one cation and two anions
In the time of dissociation give only metal cations (or NH4+), hydrogen ions and anions of acid
radical
In the time of dissociation give only metal cations (or NH4+) and anions of acid radical
Salts are:
Complex substances, which consist from atoms of metal and acid residuals
Complex substances, consisting from hydrogen atoms
Complex substances, in which atoms of metals bonded with one or several hydroxyls groups
Complex substances, consisting from two elements, one of which oxygen
Compound which molecules consist of one-type atoms
Acids are:
Complex substances, which consist from atoms of metal and acid residuals. This the most multiple
class of inorganic compounds
Complex substances, consisting of hydrogen cations and anion
Complex substances, in which atoms of metals bonded with one or several hydroxyls groups
Complex substances, consisting from two elements, one of which is oxygen
Compound which molecules consist of one-type atoms
Bases are:
Complex substances, which consist from atoms of metal and acid residuals. This the most multiple
class of inorganic compounds
Complex substances, consisting from hydrogen atoms
Complex substances, in which atoms of metals bonded with one or several hydroxyls groups
Complex substances, consisting from two elements, one of which oxygen
Compound which molecules consist of one-type atoms
Oxides are:
Complex substances, which consist from atoms of metal and acid residuals. This the most multiple
class of inorganic compounds
Complex substances, consisting from hydrogen atoms
Complex substances, in which atoms of metals bonded with one or several hydroxyls groups
Complex substances, consisting from two elements, one of which oxygen
Compound which molecules consist of one-type atoms
Monoatomic compound is:
Water
Helium
C.
D.
E.
199.
A.
B.
C. *
D.
E.
200.
A.
B.
C.
D.
E. *
201.
A.
B.
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.
Ozone
Ammonia
Oxygen
Such compound has three atoms in molecule:
Aluminum hydride
Hydrogen fluorine
Hydrogen sulfur
Ammonia
Methanol
Formula of molecule is:
ОН3O
2O
O-2
O2
Molar mass of sulfuric acid is:
49 g/mole
80 g/mole
106 g/mole
98 g/mole
65 g/mole
Mass of three mole of water is:
6g
36 g
48 g
54 g
18 g
Relative atomic mass of carbon is:
12
14
6
10
18
Molar mass of water is:
18 g
17 g/mole
24 g/mole
18 g/mole
16 g/mole
Relative atomic mass of Oxygen is:
8
15
12
18
16
Molar volume at normal stat (a temperature 273 K and pressure of 101,3 kPa) has:
A.
B. *
C.
D.
E.
207.
A.
B.
C. *
D.
E.
208.
A.
B.
C. *
D.
E.
209.
A.
B.
C.
D.
E. *
210.
A. *
B.
C.
D.
E.
211.
A.
B.
C.
D.
E. *
212.
A.
B.
C. *
D.
E.
22,4 m3
22,4 l/mol
11,2 l/mole
lest then 22,4 l/mole
more than 22,4 l/mole
During the physical phenomena:
There is a change of quantitative composition of compound
There is a change of amount of electrons in an atom
There is a change of the aggregate state of compound
There is a change only of chemical elements
There is a change of qualitative composition of molecules
112 g of nitrogen have volume:
56,9 l
11,2 l
89,6 l
112 l
22,4 l
Complex compound:
О3
C
О2
H2
СО2
Choose correct definition “simple compound is…..”
molecules or crystals are contain atoms of one element
molecules or crystals are contain atoms of 3th different elements
molecules or crystals are contain atoms of one group elements
molecules or crystals are contain atoms of 2th elements
molecules or crystals are contain atoms of different elements
To choose oxygen-containing acids:
H2S
HBr
HCl
HI
H2SO4
To choose the simple compound:
HNО3
CO
О2
H2O
СО2