Download Avogadro`s Law is relation between

1--Avogadro’s Law is relation between ………………
a-V and n at constant P,T
b- T and n at constant P,V
c-V and P at constant n,T
d- V and T at constant P, n
2-What is the difference between STP and standard molar volume?
3- Given the same number of moles of two gases at STP conditions, how
do the volumes of two gases compare?
How do the masses of the two gas samples compare?
4- How many moles of helium are contained in each volume
at STP: (a) 5.0 L; (b) 11.2 L; (c) 50.0 mL?
5- How many moles of argon are contained in each volume
at STP: (a) 4.0 L; (b) 31.2 L; (c) 120 mL?
6- Calculate the volume of each substance at STP.
a. 4.2 mol Ar b. 3.5 g CO2 c. 2.1 g N2
7- Calculate the volume of each substance at STP.
a. 4.2 mol N2 b. 6.5 g He c. 22.0 g CH4
8- What volume does 3.01 × 1021 molecules of N2 occupy
at STP?
9- What volume does 1.50 × 1024 molecules of CO2 occupy
at STP?
10-The relation between Volume of gas and its Pressure at given amount
of it and constant temperature is known as …………………
a-Boyle’s Law b- Charle’s Law
c- Avogadro’s Law d- General law
11-SF6 is a gas used in modification of eyes. If 2.5 g of this gas introduced
in evacuated 500ml container at 83°C What is the pressure in atmosphere?
a-992atm
b-0.992atm
c-9.92atm
d-99.2atm
12-Which of the following is not a common state of matter under ambient
conditions?
a-solid
b-liquid
c-plasma
13-A solid can be referred to as having
a-indefinite volume and definite shape
a-indefinite shape and definite volume
a-definite volume and definite shape
14-Molecules of a liquid have

a- strong intermolecular forces of attraction and are in a fixed position

b-weak intermolecular forces of attraction and are randomly placed
c-moderate to strong intermolecular forces of attraction and are able to shift positions
The pressure of a sample of helium in a 1.0-L container is 0.857 atm. What is the
15. new pressure if the sample is placed in a 0.5-L container? (Assume the temperature
is constant.)
a. 0.143 atm
b.
0.429 atm
c.
1.38 atm
d.
1.71 atm
16. A sample of gas is held in a 10.0-L volume at 175 kPa. The temperature is kept
constant while the volume is decreased until the pressure is 350 kPa. What is the
new volume of the gas?
a.
1.0 L
b.
5.0 L
c.
10.0 L
d.
175 L
17 A 0.5-L container of nitrogen gas is heated under constant pressure to the boiling
point of water. What is its new volume?
a. 0.5 L
b.
0.64 L
c.
0.79 L
d.
0.86 L
18. How can gases be defined?
a.
a physical state of matter that does not have a fixed shape or a fixed
volume
b.
a physical state of matter that does not have a fixed shape but has a
fixed volume
c.
a physical state of matter that has a fixed volume and a fixed shape
d.
a chemical state of matter
19. Particles of matter that are in constant, random motion and that have a size that is
much smaller than the distance between them are _____________.
a. solids
b.
liquids
c.
gases
d.
solutions
20. What is the name given to the relationship that shows that an increase in pressure
leads to a decrease in the volume of a gas?
a. Charles’s law
b.
Boyle’s law
c.
Avogadro’s number
d.
Gay-Lussac’s law
21. How can the relationship between a gas at two sets of conditions be expressed
mathematically by Boyle’s law?
a.
P1V1 = P2V2
b.
P1/V1 = P2/V2
c.
V1/T1 = V2/T2
d.
V1T1 = V2T2
22. What relationship is demonstrated by the expansion of a gas—filled balloon when it
is heated?
a. Charles’s law
b.
Boyle’s law
c.
Avogadro’s number
d.
Gay-Lussac’s law
23. A gas occupies a volume of 1.0 L at 1.0 atm pressure. What is the pressure when
the gas expands to fill 2.0 L?
a. 0.50 atm
b.
2.0 atm
c.
1.0 atm
d.
10 atm
24. A gas occupies a volume of 1.0 L at 25°C. What volume will the gas occupy at
100°C?
a. 1.0 L
b.
1.3 L
c.
0.80 L
d.
4.0 L
25. A gas occupies 2.0 L at STP. What volume will the gas occupy if the pressure is
increased to 2.0 atm, and the temperature is kept constant?
a. 1.0 L
b.
4.0 L
c.
0.50 L
d.
2.0 L
26. A sample of helium occupies 2.20 L at 1.0 atm. What is the volume at 1.5 atm?
a.
1.5 L
b.
0.68 L
c.
2.20 L
d.
1.0 L
27. When will the molecules of all samples of ideal gases have the same average
kinetic energies?
a. at constant volume
b.
at constant temperature
c.
at constant amount
d.
at constant pressure
1-The resistance of flow of a liquid is
a-wetting
b-viscosity
c-surface tension
2-The force that decreases the surface area of a liquid
a-wetting
b-viscosity
c-surface tension
3- The force bind the liquid molecules together
a-cohesion
b-adhesion
c-attraction
4- The force bind the liquid molecules and solid surface
a-cohesion
b-adhesion
c-attraction
5-If adhesion forces  the cohesion force
a-wetting
b-boiling
c-evaporation
6. This is a state of matter with a definite size or volume, but not a definite
shape.
solid
liquid
gas
7. The molecules in a liquid are
closer together than in a solid and further apart than in a gas.
are spaced the same as in solids and gases.
closer than in gases but further apart than in solids.
8. The force that holds molecules in a liquid together is called
cohesion
adhesion
surface tension
9. The process of molecules of a liquid going from the surface of a liquid into
the air is
condensation
coagulation
evaporation
10. The force that a liquid exerts on an object placed within it is called
buoyancy
condensation
1.
Consider the following reaction: 2SO2(g) + O2(g) ⇄ 2SO3(g) ∆H
= -197 kJ/mol
Which of the following will not shift the equilibrium to the right?
A.
Adding more O2
B.
Adding a catalyst
C.
Increasing the pressure
D.
Lowing the temperature
2.
Consider the following equilibrium system:
CaCO3(s) ⇄ CaO(s) + CO2(g)
Which one of the following changes would cause the above system
to shift left?
A.
B.
C.
D.
3.
Add more CaO
Remove CaCO3
Decrease volume
Increase surface area of CaO
Consider the following
equilibrium: SO2Cl2(g) + energy ⇄ SO2(g) + Cl2(g)
When the temperature is decreased, the equilibrium shifts
A.
Left and [ SO2Cl2 ] increases
B.
Left and [ SO2Cl2 ] decreases
C.
Right and [ SO2Cl2 ] increases
D.
Right and [ SO2Cl2 ] increases
Consider the following equilibrium: 2SO3(g) ⇄ 2SO2(g) + O2(g)
The volume of the system is decreased at a constant temperature. A
new state of equilibrium is established by a
shift of the original equilibrium to the
A. Left and [SO3] increases
B. Right and [SO3] decreases
C. Left and [SO3] remains unchanged
D. Right and [SO3] remains unchanged
4.
5.
Consider the following equilibrium system:
CO2(g) + H2(g) ⇄ CO(g) + H2O(g)
Which of the following, when added to the system above, would
result in a net decrease in [H2O]?
A. CO2
B. H2
C. CO
D. H2
6.
Consider the following equilibrium: C(s) + 2H2(g) ⇄ CH4(g) + 74 kJ
When a small amount of solid C is added to the system
A. [H2] decreases
B. [CH4] increases
C. The temperature increases
D. All concentrations remain constant
Consider the following equilibrium: 2NO(g) + Cl2(g) ⇄ 2NOCl(g)
At constant temperature and volume, Cl2 is added to the above
equilibrium system. As equilibrium re-establishes, the
A. [NOCl] will decrease
B. The temperature increases
7.
C. [NO] will increase
D. [NOCl] will increase
8.
Consider the following
equilibrium: Cl2O7(g) +8H2(g) ⇄ 2HCl(g) + 7H2O(g)
Which of the following would increase the number of moles of HCl?
A. Increase [H2O]
B. Increase [Cl2O7]
C. Increase total pressure
D. Increase volume of the system
9.
Consider the following
equilibrium: 2HI(g) ⇄
H2(g) + I2(g) ∆H = -68kJ
Which of the following would cause the equilibrium to shift right?
A. Increasing the volume
B. Decreasing the volume
C. Increasing the temperature
D. Decreasing the temperature
10.
A 1.00 L flask contains a gaseous equilibrium system. The addition
of reactants to this flask results in a
A. Shift to the left and decrease in the concentration of products
B. Shift to the left and increase in the concentration of products
C. Shift to the right and decrease in the concentration of products
D. Shift to the right and increase in the concentration of products
11.
When the temperature of an equilibrium system is increased, the
equilibrium always shifts to favor the
A. Exothermic reaction
B. Endothermic reaction
C. Formation of products
D. Formation of reactants
12.
An equilibrium system shifts left when the
A. Rate of the forward reaction is equal to the rate of the reverse
reaction
B. Rate of the forward reaction is less than the rate of the reverse
reaction
C. Rate of the forward reaction is greater than the rate of the reverse
reaction
A. Rate of the forward reaction and the rate of the reverse reaction
are constant
13.
Consider the following
equilibrium: 2SO2(g) + O2(g) ⇄ 2SO3(g) ∆H = -198 kJ
There will be no shift in the equilibrium when
A. More O2 is added
B. Catalyst is added
C. The volume is increased
D. The temperature is increased
Consider the following equilibrium: 2NOCl(g) ⇄ 2NO(g) + Cl2(g)
In a 1.0 L container at equilibrium there are 1.0 mol NOCl, 0.70 mol
NO and 0.40 mol Cl2.
At constant temperature and volume, 0.10 mol NOCl is added. The
concentrations in the
“new” equilibrium in comparison to the concentrations in the “old”
equilibrium are
14.
A.
B.
C.
D.
[NOCl]
new = old
new > old
new < old
new < old
[NO]
new = old
new > old
new < old
new > old
[Cl2]
new = old
new > old
new > old
new > old
15.
Consider the following equilibrium: N2O4(g) + 58 kJ ⇄ 2NO2(g)
The equilibrium shifts right when
A. NO2 is added
B. N2O4 is removed
C. The temperature is decreased
D. The volume of the system is increased
16.
Consider the following equilibrium: 2SO2(g) + O2(g) ⇄ 2SO 3(g)
Which of the following will shift the equilibrium to the right?
I. Adding more O2
II. Adding more SO3
III. Adding a catalyst
A. I only
B. III only
C. I and II only
D. II and III only
17.
Consider the following equilibrium:
energy + 2NaClO3(s) ⇌ 2NaCl(s) + 3O2(g)
Which of the following will cause a shift to the left?
A.
adding more O2
B.
adding more NaCl
C.
removing some NaClO3
D.
increasing the temperature
18.
Consider the following equilibrium:
CO(g) + 2H2(g) ⇌ CH3OH(g) + energy
Which of the factors below would decrease the concentration of
CH3OH at equilibrium?
A.
an addition of CO
B.
an increase in H2
C.
a decrease in the temperature
D.
an increase in the temperature
19.
Consider the following equilibrium:
energy + 2NaClO3(s) ⇌ 2NaCl(s) + 3O2(g)
Which of the following will cause a shift to the right?
A.
adding more O2
B.
adding more NaCl
C.
removing some NaCl(s)
D.
increasing the temperature
20.
Consider the following equilibrium: 2SO2(g) + O2(g) ⇄ 2SO 3(g)
Which of the following will shift the equilibrium to the left?
I. Removing O2
II. Adding more SO3
III. Adding a catalyst
A.
B.
C.
D.
21.
I only
III only
I and II only
II and III only
Consider the following
equilibrium: N2O4(g) + energy ⇌ 2NO2(g)
How are N2O4 and NO2 affected by the addition of He into the
container at constant volume.
N2O 4
NO2
A.
no change
no change
B.
no change
increases
C.
increases
decreases
D.
decreases
increases
22.
Which of the following stresses will cause a shift to the reactants?
H2(g) + Br2(g) ⇌ 2HBr(g) + energy
A.
increase [Br2]
B.
increase [H2]
C.
decrease temperature
D.
increase temperature
23.
Which of the following stresses will cause a shift to the products?
H2(g) + Br2(g) ⇌ 2HBr(g) + energy
A.
decrease [Br2]
B.
decrease [H2]
C.
decrease temperature
D.
increase temperature
24.
Which of the following two stresses will each cause the system to
shift to the left?
2SO2(g) + O2(g) ⇄ 2SO 3(g) + energy
A.
decrease temperature and decrease [O2]
B.
C.
D.
increase temperature and increase [SO3]
increase temperature and decrease [SO3]
decrease temperature and increase [SO2]
SrCO3(s) + 215 kJ ⇌ SrO(s) + CO2(g)
Which of the following conditions would produce the greatest yield
of SrO(s)?
Temperature
Pressure
A.
low
low
B.
low
high
C.
high
low
D.
high
high
25.
26.
The Haber Process is used to produce ammonia commercially
according to the following equilibrium:
N2(g) + 3H2(g) ⇌ 2NH3(g) + energy
Which of the following conditions will produce the highest yield
of ammonia?
A.
increase temperature and increase pressure
B.
increase temperature and decrease pressure
C.
decrease temperature and increase pressure
D.
decrease temperature and decrease pressure
27.
Consider the following reaction: 2SO2(g) + O2(g) ⇄ 2SO3(g) ∆H
= -197 kJ/mol
If the volume is increased what happens to position of the
equilibrium?
A.
shifts to the right
B.
shifts to the left
C.
no shift
D.
shifts in the exothermic direction
28.
Consider the following reaction: 2NH3(g) +
energy ⇄ N2(g) + 3H2(g)
If the volume is increased what happens to position of the
equilibrium?
A.
shifts to the right
B.
shifts to the left
C.
no shift
D.
shifts in the exothermic direction
29.
Consider the following reaction:
SrCO3(s) + 215 kJ ⇌ SrO(s)
+ CO2(g)
If the volume is decreased what happens to position of the
equilibrium?
A.
shifts to the right
B.
shifts to the left
C.
no shift
D.
shifts in the exothermic direction
30.
Consider the following
reaction: H2(g) + Br2(g) ⇌ 2HBr(g) + energy
If the volume is increased what happens to position of the
equilibrium?
A.
shifts to the right
B.
shifts to the left
C.
no shift
D.
shifts in the exothermic direction
Consider the following reaction: N2O4(g) + energy ⇌ 2NO2(g)
If the volume is decreased what happens to position of the
equilibrium?
A.
shifts to the right
B.
shifts to the left
C.
no shift
D.
shifts in the exothermic direction
31.
1-Compounds that ionized completely in solution
a-non-electrolyte
b-strong electrolyte c-weak electrolyte
2- Strong base solution are considered
a-non-electrolyte
b-strong electrolyte c-weak electrolyte
+
3-The negative logarithm of the H ion concentration
a- pKa
b- pH
c-pOH
4-The solution composed of weak acid and its salt
a-buffer
b-neutral
5-The Na2CO3 salt is ……………… salt type
c- electrolyte
a-acidic
b- basic
c- neutral
b-14
c-1014
6-The sum of pH and pOH
a- 7
7- Calculate the value of [–OH] from the given [H3O+] and label the
solution as acidic or basic.
a. 10–8 M c. 3.0 × 10–4 M
b. 10–10 M d. 2.5 × 10–11 M
8- Calculate the value of [–OH] from the given [H3O+] and
label the solution as acidic or basic.
a. 10–1 M c. 2.6 × 10–7 M
b. 10–13 M d. 1.2 × 10–12 M
9- Calculate the value of [H3O+] from the given [–OH] and
label the solution as acidic or basic.
a. 10–2 M c. 6.2 × 10–7 M
b. 4.0 × 10–8 M d. 8.5 × 10–13 M
10- Calculate the value of [H3O+] from the given [–OH] and
label the solution as acidic or basic.
a. 10–12 M c. 6.0 × 10–4 M
b. 5.0 × 10–10 M d. 8.9 × 10–11 M
11- Calculate the pH from each H3O+ concentration
calculated in Problem 9.77.
12- Calculate the pH from each H3O+ concentration
calculated in Problem 9.78.
13- Calculate the H3O+ concentration from each pH: (a) 12;
(b) 1; (c) 1.80; (d) 8.90.
14- Calculate the H3O+ concentration from each pH: (a) 4;
(b) 8; (c) 2.60; (d) 11.30.
15- If a urine sample has a pH of 5.90, calculate the concentrations of
H3O+ and –OH in the sample.
16- If pancreatic fl uids have a pH of 8.2, calculate the concentrations of
H3O+ and –OH in the pancreas.
17- Determine whether each salt forms an acidic, basic, or
neutral solution when it dissolves in water.
a. NaI
c. NH4NO3
b. LiF
d. KHCO3
e. MgBr2
f. NaH2PO4
18- Determine whether each salt forms an acidic, basic, or
neutral solution when it dissolves in water.
a. NaBr
c. KCH3COO
b. NaCN
d. CsF
e. CaBr2
f. K3PO4
19-The pH of a solution contain0.05 M H+ concentration
a-5
b-1.3
c-3.1
20-The pH of a solution contain M OH- concentration
a-1.3
b-12.7
c-3.1
1- Write the ion symbol for an atom with the given number
of protons and electrons.
a. four protons and two electrons
b. 22 protons and 20 electrons
c. 16 protons and 18 electrons
d. 13 protons and 10 electrons
e. 17 protons and 18 electrons
f. 20 protons and 18 electrons
2- How many protons and electrons are present in each ion?
a. K+ b. S2– c. Mn2+ d. Fe2+ e. Cs+ f. I–
3- What element fi ts each description?
a. a period 2 element that forms a +2 cation
b. an ion from group 7A with 18 electrons
c. a cation from group 1A with 36 electrons
4-Give the ion symbol for each ion.
a. sodium ion c. manganese ion e. stannic
b. selenide d. gold(III)
5- Give the ion symbol for each ion.
a. barium ion c. oxide e. lead(IV)
b. iron(II) d. ferrous
6- What noble gas has the same electronic confi guration as
each ion?
a. O2– b. Mg2+ c. Al3+ d. S2– e. F– f. Be2+
7- Give two cations and two anions that have the same electronic confi
guration as each noble gas:
(a) neon;
(b) argon.
8- How many electrons must be gained or lost by each element to achieve
a noble gas confi guration of electrons?
a. lithium b. iodine c. sulfur d. strontium
9- How many electrons must be gained or lost by each
element to achieve a noble gas confi guration of electrons?
a. cesium b. barium c. selenium d. aluminum
10- Which ions are likely to form? For those ions that are not
likely to form, explain why this is so.
a. S– b. S2– c. S3– d. Na+ e. Na2+ f. Na–
11- Which ions are likely to form? For those ions that are not
likely to form, explain why this is so.
a. Mg+ b. Mg2+ c. Mg3+
d. Cl+
e. Cl–
f. Cl2–
1-Give the name of the elements in each group of three element symbols.
a. Au, At, Ag d. Ca, Cr, Cl
b. N, Na, Ni e. P, Pb, Pt
c. S, Si, Sn f. Ti, Ta, Tl
2- What element(s) are designated by each symbol or group
of symbols?
a. CU and Cu c. Ni and NI
b. Os and OS d. BIN, BiN, and BIn
3- Does each chemical formula represent an element or a
compound?
a. H2 b. H2O2 c. S8 d. Na2CO3 e. C60
4- Identify the elements in each chemical formula and tell how many
atoms of each are present.
a. K2Cr2O7
b. C5H8NNaO4 (MSG, fl avor enhancer)
c. C10H16N2O3S (vitamin B7)
5- Identify the element that fi ts each description.
a. an alkali metal in period 6
b. a transition metal in period 5, group 8
c. a main group element in period 3, group 7A
d. a main group element in period 2, group 2A
e. a halogen in period 2
f. an inner transition metal with one 4f electron
6- Identify the element that fi ts each description.
a. an alkaline earth element in period 3
b. a noble gas in period 6
c. a main group element in period 3 that has p orbitals
half-fi lled with electrons
d. a transition metal in period 4, group 11
e. an inner transition metal with its 5f orbitals completely
f. a transition metal in period 6, group 10 filled with electrons
7- Label each region on the periodic table.
a. noble gases e. alkaline earth elements
b. period 3 f. f block elements
c. group 4A g. transition metals
d. s block elements h. group 10
8- Identify each highlighted element in the periodic table
and give its [1] element name and symbol; [2] group number; [3] period;
[4] classifi cation (i.e., main group element, transition metal, or inner
transition metal).
9-Write the element symbol that fi ts each description, using
a superscript for the mass number and a subscript for the
atomic number.
a. an element that contains 53 protons and 74 neutrons
b. an element with 35 electrons and a mass number of 79
c. an element with 47 protons and 60 neutrons
10- Which element in each pair is larger?
a. bromine and iodine c. silicon and potassium
b. carbon and nitrogen d. chlorine and selenium
11- Which element in each pair has its valence electrons
farther from the nucleus?
a. sodium and magnesium c. neon and krypton
b. carbon and fl uorine d. argon and bromine
12- Give the number of valence electrons in each element.
Write out the electronic confi guration for the valence
electrons.
a. sulfur b. chlorine c. barium d. titanium e. tin
13- Give the number of valence electrons in each element.
Write out the electronic confi guration for the valence
electrons.
a. neon c. aluminum e. zirconium
b. rubidium d. manganese
14-What is the maximum number of electrons that can be
contained in each shell, subshell, or orbital?
a. second shell c. 3p subshell e. fourth shell
b. 3s orbital d. 4f orbital f. 5p orbital
15-Write the element symbol that fi ts each description. Use a superscript
for the mass number and a subscript for the atomic number.
a. an element that contains 10 protons and 12 neutrons
b. an element with atomic number 24 and mass
number 52
16-How many protons, neutrons, and electrons are contained
in each element?
a. 27 13Al b. 35
17Cl
c. 3416S
17-Give all of the terms that apply to each element:
[1] metal; [2] nonmetal; [3] metalloid; [4] alkali metal;
[5] alkaline earth element; [6] halogen; [7] noble gas;
[8] main group element; [9] transition metal; [10] inner
transition metal.
a. sodium c. xenon e. uranium
b. silver d. platinum f. tellurium
18- Give all of the terms that apply to each element:
[1] metal; [2] nonmetal; [3] metalloid; [4] alkali metal;
[5] alkaline earth element; [6] halogen; [7] noble gas;
[8] main group element; [9] transition metal; [10] inner
transition metal.
a. bromine c. cesium e. calcium
b. silicon d. gold f. chromium
19-For the given atomic number (Z) and mass number (A):
[1] identify the element; [2] give the element symbol;
[3] give the number of protons, neutrons, and electrons.
a. Z = 10, A = 20 d. Z = 55, A = 133
b. Z = 13, A = 27 e. Z = 28, A = 59
c. Z = 38, A = 88 f. Z = 79, A = 197
20-Give the name of the elements in each group of three
element symbols.
a. Au, At, Ag
d. Ca, Cr, Cl
b. N, Na, Ni
e. P, Pb, Pt
c. S, Si, Sn
f. Ti, Ta, Tl
1- Which formulas represent ionic compounds and which
represent covalent compounds?
a. CO2 b. H2SO4 c. KF d. CH5N
2- Which formulas represent ionic compounds and which
represent covalent compounds?
a. C3H8 b. ClBr c. CuO d. CH4O
3- Which pairs of elements are likely to form ionic bonds
and which pairs are likely to form covalent bonds?
a. potassium and oxygen c. two bromine atoms
b. sulfur and carbon d. carbon and oxygen
4- Which pairs of elements are likely to form ionic bonds
and which pairs are likely to form covalent bonds?
a. carbon and hydrogen c. hydrogen and oxygen
b. sodium and sulfur d. magnesium and bromine
5- Why do ionic bonds form between a metal and a
nonmetal?
6- How many electrons must each atom gain or lose to acquire an
electron configuration identical to the noble gas neareast to it in atomic
number
a-Li
b- Cl
e- Sr
f- S
c-P
g-Si
d- Al
h- O
1- Convert each compound to a condensed structure.
2- Convert each compound to a condensed structure.
3-Convert each compound to a skeletal structure.
4- Convert each compound to a skeletal structure.
5- Convert each shorthand structure to a complete structure
with all atoms and lone pairs drawn in.
6-Convert each shorthand structure to a complete structure with all atoms
and lone pairs drawn in.
7-What is wrong in each of the following shorthand structures?
8-
9-
10-
Functional Groups
Identify the functional groups in each molecule.
11-
1-Which quantity has the greater mass?
a. 1 mol of Si atoms or 1 mol of Ar atoms
b. 1 mol of He atoms or 6.02 × 1023 H atoms
c. 1 mol of Cl atoms or 1 mol of Cl2 molecules
d. 1 mol of C2H4 molecules or 3.01 × 1023 C2H4
molecules
2- How many grams are contained in 5.00 mol of each
compound?
a. HCl b. Na2SO4 c. C2H2 d. Al(OH)3
3- How many grams are contained in 0.50 mol of each
compound?
a. NaOH b. CaSO4 c. C3H6 d. Mg(OH)2
4- How many moles are contained in each number of grams
of table sugar (C12H22O11, molar mass 342.3 g/mol)?
a. 0.500 g b. 5.00 g c. 25.0 g d. 0.0250 g
5- How many moles are contained in each number of
grams of fructose (C6H12O6, molar mass 180.2 g/mol), a
carbohydrate that is about twice as sweet as table sugar?
“Lite” food products use half as much fructose as table
sugar to achieve the same sweet taste, but with fewer
calories.
a. 0.500 g b. 5.00 g c. 25.0 g d. 0.0250 g
6- Which has the greater mass: 0.050 mol of aspirin or
10.0 g of aspirin (C9H8O4)?
7- What is the mass in grams of 2.02 × 1020 molecules
of the pain reliever ibuprofen (C13H18O2, molar mass
206.3 g/mol)?
8- How many molecules of butane (C4H10) are contained in
the following number of moles: (a) 2.00 mol; (b) 0.250 mol;
(c) 26.5 mol; (d) 222 mol; (e) 5.00 × 105 mol?
9- How many moles of pentane (C5H12) are contained in the
following number of molecules?
a. 5.00 × 1019 molecules c. 8.32 × 1021 molecules
b. 6.51 × 1028 molecules d. 3.10 × 1020 molecules
10- What is the mass in grams of each quantity of lactic
acid (C3H6O3, molar mass 90.1 g/mol), the compound
responsible for the aching feeling of tired muscles during
vigorous exercise?
a. 3.60 mol c. 7.3 × 1024 molecules
b. 0.580 mol d. 6.56 × 1022 molecules
11- What is the mass in grams of each quantity of vitamin D
(molar mass 384.7 g/mol), which is needed for forming
and maintaining healthy bones?
a. 3.6 mol c. 7.3 × 1024 molecules
b. 0.58 mol d. 6.56 × 1022 molecules
12-Identify the species that is oxidized and the species that is reduced in
each reaction. Write out two half reactions to show how many electrons
are gained or lost by each species.
10-The following elements F, Cl, Br show similarity in
chemical, physical properties because …….
a-they arein periodic table
c-they are in same period
b- they are in same group
d-they are metals
11-The Empirical formula of glucose C6H12O6 is …………….
a-C6H12O6b- C2H4O2
c-CHO
d- CH2O
12- The formula of ionic compound formed by Mg2+ and NO3- is
……..
a-MgNO3
b-Mg2NO3
c- Mg(NO3)2 d-Mg2(NO3)2
13-The difference between the isotopes of same element is in
number of
a-Protons
b- Electrons
c-Atomic number
d-
Neutrons
14-The mass of one atom of Se78.96metal in gram is ……….
Note: Avogadro’s number =6.02˟ 1023
a-1.13˟ 10-22 b-1.311˟ 1022
c-131˟ 10-22
d-13˟ 10-24
15-How many moles of carbon are present in 0.8 mole of
C6H12O6?
a-6 mole
b- 4 mole
c- 4.8 mole
d-
0.8 mole
16-The mass percent of H atom in NaHCO3 is ………….
a-1.19%
21.9%
b- 2.19%
c- 11.9%
d-