Practice Exam 2 – 75 minute2
Chapters 5, 6, 13
Useful Information
Constants
1 atm = 760 mm Hg = 760 torr
R =
0.08206 L.atm/mol.K = 8.315 J/mol.K
NA = 6.022 x 1023 (Avagadro’s Number)
specific heat of water = 4.184
J/g.K
Van der
Waal’s Equation
Ek = 1/2 mu2 = 3/2 kT
per molecule
Ek = ½ Mu2
= 3/2 RT per mole
=
Rate of Effusion2
Rate of Effusion1
=
Kp = Kc(RT)Dn where Dn = mol product
gas-mol reactant gas
Multiple Choice (2 points
each)
_____1. The value of ∆E for a system that does 213 kJ
of work on its surroundings and loses 79 kJ of heat is _______kJ.
A) +292 B) -292 C) +134 D)
-134 E) -213
_____2. When NH4Cl(s) dissolves in water the
solution formed shows a decrease in temperature (a “cold pack”). This solution process is ____________ and has
a ________ΔH.
A) endothermic, negative
B) endothermic,
positive
C) exothermic,
negative
D) exothermic,
positive
E) cannot
be determined from the information given
_____3. Given the thermochemical
equation
2 SO2(g) + O2(g) →
2 SO3(g) ∆H = -198
kJ
What is the enthalpy change, ∆H,
for the decomposition of one mole of SO3 into SO2 and O2?
A) 198 kJ
B) -99 kJ C) 99 kJ
D) 396 kJ E)
-198 kJ
_____4. The standard enthalpy of formation, DH°f, for nitrogen dioxide is the enthalpy change for the reaction
A) N(g)
+ 2O(g) à NO2(g)
B) 1/2 N2(g)
+ O2(g) àNO2(g)
C) NO(g)
+ O(g) à NO2(g)
D) NO(g)
+ 1/2 O2(g) àNO2(g)
_____5. If the temperature
of a particular sample of gas is tripled and its volume doubled, what will the
new pressure be?
A)
2/3 Poriginal B)1/6 Poriginal C) 3/2 Poriginal D)
6 Poriginal E) no change
_____6.Which set of conditions
would give the least ideal gas
conditions?
A)
High temperature, high pressure
B)
High temperature, low pressure
C)
Low temperature, low pressure
D)
Low temperature, high pressure
E)
Does not matter; all
gases behave ideally.
_____7. What is the ratio of the rates of effusion of H2O(g) to D2O(g)? (molar
mass D2O = 20.0 g/mol)
A) 0.900 B) 0.950 C) 1.05 D)
1.11
_____8. Consider a reaction 2 A(s) + B(g)
Û 2 C(g). If 0.20 mol A, 0.30 mol B and 0.10 mol C are present in a 1.0 L flask at
equilibrium, what is Kc?
A) 0.033 B) 0.83 C) 1.7 D)
30. E) none of the above
_____9. This reaction occurs readily above 500 °C.
2HgO(s) Û2Hg(l) + O2(g)
What is the equilibrium
constant expression for this reaction?
A) K = [Hg]2[O2] / [HgO]2
B) K = [Hg][O2] / [HgO]
C) K = [Hg]2[O2]
D) K = [O2]
_____10. Which reaction characteristics will be affected by a
change in temperature?
1. value of equilibrium constant
2. equilibrium
concentrations
A) 1 only
B) 2 only
C) 1 and 2
D) neither 1 nor 2
11. (6 pts) Equal
masses of helium and neon are placed in separate containers of equal volume at
the same temperature. Circle the correct answer for each part.
i.
Pressures of the
gases.
a. The pressure of helium is greater than the
pressure of neon.
b.
The pressure of
neon is greater than the pressure of helium.
c.
The pressures of
the gases are the same.
ii. Energies of the atoms
- The average energy of helium atoms is greater
than that of neon atoms
- The average energy of neon atoms is greater than that
of helium atoms.
- The average energy of helium atoms is the same as that
of neon atoms.
iii.
Speeds of the
atoms.
a. The average
speed of helium
atoms is greater than that of neon atoms
b. The average
speed of neon
atoms is greater than that of helium
atoms
c. The average
speed of neon
atoms is the same as that of helium
atoms
12.
(7 pts) Given the two equilibrium below (I & II),
what is the Keq for:
Zn3(PO4)2 (s)
+ 12
(I) 3 Zn2+ (aq) + 2 PO43– (aq)
<––––> Zn3(PO4)2
(s) KI = 1.1 x 1032
(II) Zn2+ (aq) + 4
13. (7 pts) Given these values of DH°:
CS2(l)
+ 3O2(g) à CO2(g) + 2SO2(g) DH° = - 1077 kJ
H2(g)
+ O2(g) à H2O2(l) DH° = - 188 kJ
H2(g)
+ 1/2 O2(g) à H2O(l) DH° = - 286 kJ
What is the value of DH° for this reaction?
CS2(l)
+ 6H2O2(l) à CO2(g) + 6H2O(l) + 2SO2(g)
14. (10 pts) An alloy of aluminum and copper is analyzed for percentage
composition. A 0.2052 g sample of the alloy is dissolved in sulfuric acid
(copper does not react with sulfuric acid) and 229.5 mL
of hydrogen gas are collected at 700. torr
and 29 oC. The balanced equation is
2 Al + 3H2SO4
à Al2(SO4)3
+ 3 H2
Calculate the percentage of
aluminum in the alloy.
15. (7 pts) When 2.75 mol HI(g) are placed into a 1.00-L container at 25 °C and
allowed to dissociate according to the equation:
2 HI (g) Û H2(g) + I2(g)
The final concentration of H2(g) is found to be 0.275 M. What is the Kc for the reaction?
16. (7 pts) At a certain temperature K = 6.3 x 107 for the
reaction
2NO(g) +
Cl2(g) Û 2NOCl(g)
Calculate the concentration
of NO at equilibrium if 2.0 moles of NO and 1.0 mole of Cl2 are
placed in a 1.0 L flask.
17. (8 pts) Calculate the
molar mass of the
compound if the 1.103 g sample occupies a volume of 582 mL
at 765.5 torr and 25.00oC.
18. (10 pts) Ammonium carbamate, NH2COONH4, is a salt found
in the blood and urine of mammals. At
520 K, KC
is 1.58 x 10-8 for the following
equilibrium:
NH2COONH4(s) Û
2NH3(g) + CO2(g)
If 7.80 g of NH2COONH4
is introduced into a 0.500 L evacuated container at 520 K, what will be the
total pressure inside the container at equilibrium?
19.
(8 pts) The enthalpy of neutralization, DH, of HCl (aq) by NaOH(aq)
is -55.90 kJ/mol H2O produced.
If 50.00 mL of 1.05 M NaOH
is added to 25.00 mL of 1.86 M HCl,
with both solutions originally at 24.72 oC,
what will be the final solution temperature?
Assume no heat is lost to the surrounding air and that the aqueous
solution has a density of 1.02 g/mL and a specific
heat of 3.98 J/g . oC.
20. (10 pts) For this reaction at equilibrium, how will the indicated
changes affect the equilibrium? Fe3O4(s)
+ 4 H2(g) Û 3 Fe(s) + 4 H2O(g) DH > 0
A)
|
Change to system at equilibrium |
Shift to re-establish equilibrium (left, right, or no change) |
Amount of Fe(s) present in the system |
|
increasing temperature |
|
|
|
adding H2 |
|
|
|
adding Fe(s) |
|
|
|
Decrease volume of container |
|
|
B) How will increasing the
temperature affect the value of the equilibrium constant, K, for reaction?