Download Equilibrium Multiple Choice

Equilibrium Multiple Choice
January 1999
7. Consider the following graph:
When equilibrium is reached, the rate of the forward reaction is
A. 0.00 mol/min
B. 0.25mol/min
C. 1.0 mol/min
D. 3.0 mol/min
8. Consider the following equilibrium:
2NO2 (g)
N2O4 (g) + energy
The equilibrium will shift to the left as a result of
A. adding a catalyst.
B. increasing the volume.
C. removing some N2O4.
D. decreasing the temperature.
9. Ethene, C2H4, can be produced in the following industrial system:
C2H6 (g) + energy
C2H4 (g) + H2 (g)
The conditions that are necessary to maximize the equilibrium yield of C2H4 are
A. low temperature and low pressure.
B. low temperature and high pressure.
C. high temperature and low pressure.
D. high temperature and high pressure.
10. Consider the following equilibrium:
H2 (g) + I2 (g)
2HI (g)
The volume of the equilibrium system is increased and a new equilibrium is established.
Compared to the rates in the original equilibrium, which of the following describes the
rates of the forward and reverse reactions in the new equilibrium?
11. Consider the following equilibrium:
N2 (g) + 3H2 (g)
2NH3 (g) + energy
Certain conditions provide less than 10% yield of NH3 at equilibrium. Which of the
following describes this equilibrium?
12. Which of the following best describes the relationship between Keq and temperature
for an endothermic reaction?
April 1999
7. Consider the following PE diagram for a reversible reaction:
Which of the following describes this reaction?
8. Consider the following equilibrium:
2NO(g) + Br2(g) + energy
The equilibrium will shift to the left as a result of
2NOBr(g)
A. adding a catalyst.
B. removing NOBr.
C. increasing the volume.
D. increasing the temperature.
9. Consider the following equilibrium:
N2(g) + O2(g) + energy
2NO(g)
When the temperature is increased, the equilibrium shifts to the
A. left and Keq increases.
B. left and Keq decreases.
C. right and Keq increases.
D. right and Keq decreases.
10. Consider the following equilibrium:
2CO(g) + O2(g)
2CO2 (g) + energy
Some CO2 is added to the equilibrium system at constant volume and a new equilibrium
is established. Compared to the original equilibrium, the rates of the forward and reverse
reactions for the new equilibrium have
11. An indication that an equilibrium system favours the products is a
A. large Keq .
B. positive ∆H.
C. one step mechanism.
D. low activation energy.
12. The relationship between Keq and the pressure of a gaseous equilibrium at constant
temperature can be described by
13. Consider the following equilibrium:
2NO2(g)
N2O4(g)
A 1.00 L flask contains 0.030 mol NO2 and 0.040 mol N2O4 at equilibrium.
The value of Keq is
A. 0.023
B. 0.67
C. 1.3
D. 44
June 1999
7. Consider the following reaction:
N2(g) + 3H2(g) 2NH3 (g) + energy
Which of the following describes the changes in enthalpy and entropy as the reaction
proceeds?
8. Consider the following equilibrium:
2SO2(g) + O2(g)
2SO3(g) + energy
Which of the following will cause this equilibrium to shift to the left?
A. adding a catalyst
B. adding some SO2
C. increasing the volume
D. decreasing the temperature
9. Methanol, CH3OH, can be produced by the following:
CO(g) + 2H2(g)
CH3OH(g) + energy
The conditions that are necessary to maximize the equilibrium yield of CH3OH are
A. low temperature and low pressure.
B. high temperature and low pressure.
C. low temperature and high pressure.
D. high temperature and high pressure.
10. A catalyst is added to a system already at equilibrium. How are the forward and
reverse reaction rates affected by the addition of the catalyst?
11. Consider the following reaction:
2H2(g) + O2(g)
2H2O(l)
What is the equilibrium constant expression for the reaction?
A. Keq = [H2]2[O2]
[H2]2[O2]
B. Keq= --------------[H2O]2
[H2O]2
C. Keq= --------------[H2]2[O2]
1
D. Keq= -----------------[H2]2[O2]
12. The relationship between Keq and temperature for an exothermic reaction is
represented by
13. Consider the following equilibrium:
2NOBr(g)
2NO(g) + Br2(g)
Keq = 6.4 X 10-2
At equilibrium, a 1.00 L flask contains 0.030 mol NOBr and 0.030 mol NO.
How many mol Br2 are present?
A. 1.9 ×10−3 mol
B. 6.4 ×10−2 mol
C. 3.0 ×10−2 mol
D. 4.7 ×10−1 mol
August 1999
7. At different conditions, the relationship between the forward and reverse rates of
reaction in an equilibrium system can be represented by
8. Consider the following equilibrium:
4NH3(g) + 5O2(g)
4NO(g) + 6H2O (g) + energy
Which of the following will cause the equilibrium to shift to the left?
A. adding H2O(g)
B. removing some NO (g)
C. increasing the volume
D. decreasing the temperature
9. Consider the following equilibrium:
2NO(g) + O2(g)
2NO2 (g) + energy
When the volume of the container is increased, the equilibrium shifts to the
A. left and Keq decreases.
B. right and Keq increases.
C. left and Keq remains constant.
D. right and Keq remains constant.
10. Consider the following equilibrium:
4HCl (g) + O2(g)
2H2O(g) + 2Cl2 (g) + energy
The temperature of the equilibrium system is increased and a new equilibrium is
established. The rates of the forward and reverse reactions for the new equilibrium
compared to the original equilibrium have
11. Consider the following reaction:
2Hg(g) + O2(g)
2HgO(s)
The equilibrium constant expression for the reaction is
12. The value of Keq changes when
A. a catalyst is added.
B. the temperature changes.
C. the surface area changes.
D. the concentration of reactants changes.
13. Consider the following equilibrium:
PCl5(g)
PCl3(g) + Cl2(g)
A 1.00 L flask contains 0.0200 mol PCl5, 0.0500 mol PCl3 and 0.0500 mol Cl2 at
equilibrium. The value of Keq is
A. 0.125
B. 2.50
C. 5.00
D. 8.00
January 2000
7. Consider the following equilibrium:
N2(g) + 2O2(g)
2NO2(g)
Equal moles of N2 and O2 are added, under certain conditions, to a closed container.
Which of the following describes the changes in the reverse reaction which occur as the
system proceeds toward equilibrium?
8. A chemical equilibrium is described as “dynamic” because
A. maximum randomness has been achieved.
B. the pressure and temperature do not change.
C. both reactants and products continue to form.
D. the concentrations of chemical species remain constant.
9. Which of the following reactions results in an entropy increase?
A. 2C(s) + O2(g) 2CO(g)
B. N2(g) + 2H2(g) N2H4(l)
C. 2SO2(g) + O2(g) 2SO3(g)
D. Ag+ (aq) + Cl- (aq) AgCl(s)
10. Consider the following equilibrium:
CH3COOH(aq) + H2O(l)
CH3COO- (aq) + H3O+ (aq) + heat
A stress was applied at time t1 and the data was plotted on the following graph:
The stress that was imposed at time t1 is the result of
A. the addition of HCl.
B. decreasing the temperature.
C. the addition of NaCH3COO.
D. increasing the volume of the container.
11. Consider the following potential energy diagram for an equilibrium system:
When the temperature of the system is increased, the equilibrium shifts to the
A. left and the Keq increases.
B. left and the Keq decreases.
C. right and the Keq increases.
D. right and the Keq decreases.
12. What is the Keq expression for the following equilibrium?
Fe3O4(s) + 4H2(g)
3Fe(s) + 4H2O(g)
13. Consider the following equilibrium:
2O3(g)
3O2(g)
Keq= 65
Initially, 0.10 mole of O3 and 0.10 mole of O2 are placed in a 1.0L container. Which of
the following describes the changes in concentrations as the reaction proceeds toward
equilibrium?
April 2000
7. Which of the following applies to a chemical equilibrium?
I.
II.
III.
Forward and reverse reaction rates are equal
Equilibrium can be achieved from either direction
Macroscopic properties are constant
A. I only
B. I and II only
C. II and III only
D. I, II and III
8. In which of the following will the driving forces of minimum enthalpy and maximum
entropy oppose one another?
A. 2C(s) + O2(g) 2CO(g)
B. 2N2(g) + O2(g) 2N2O(g)
C. 2CO(g) + O2(g) 2CO2(g)
D. 2CO2(g) + 6H2O(g) 2C2H6(g) + 7O2(g)
∆H= -221kJ
∆H= +164kJ
∆H= -566kJ
∆H= +3122kJ
9. Consider the following equilibrium:
2CrO4 2- (aq) + 2H3O+ (aq)
(yellow)
Cr2O7 2- (aq) + 3H2O(l)
(orange)
An unknown solution is added to an orange equilibrium sample until the sample turns
yellow. The unknown solution could be
A. KNO3
B. NaOH
C. NH4NO3
D. CH3COOH
10. Ammonia, NH3 , is produced by the following reaction:
N2(g) + 3H2(g)
2NH3(g) + energy
Which of the following would result in the highest concentration of ammonia at
equilibrium?
A. increasing the temperature and increasing the pressure
B. decreasing the temperature and increasing the pressure
C. increasing the temperature and decreasing the pressure
D. decreasing the temperature and decreasing the pressure
11. What is the Keq expression for the following reaction?
SnO2(s) + 2CO(g)
Sn(s) + 2CO2(g)
12. Consider the following reaction:
C(s) + 2H2(g)
CH4(g)
∆H = -74.8KJ
Which of the following will cause an increase in the value of Keq?
A. increasing [H2]
B. decreasing the volume
C. finely powdering the C (s)
D. decreasing the temperature
13. Consider the following equilibrium:
H2(g) + I2(g)
2HI(g)
At equilibrium [H2] = 0.00220 mol/L, [I2] = 0.00220 mol/L and [HI] = 0.0156mol/L.
The value of Keq is
A. 3.10 X 10-4
B. 1.99 X 10-2
C. 5.03 X 101
D. 3.22 X 103
June 2000
7. Consider the following equilibrium:
2NOCl(g)
2NO(g) + Cl2(g)
A flask of fixed volume is initially filled with NOCl(g), NO(g) and Cl2(g) . When
equilibrium is reached, the pressure has increased. To reach equilibrium, the reaction
proceeded to the
A.
B.
C.
D.
left because Trial Keq was less than Keq.
right because Trial Keq was less than Keq.
left because Trial Keq was greater than Keq .
right because Trial Keq was greater than Keq .
8. In which of the following do both minimum enthalpy and maximum entropy factors
favour the reactants?
A. Cl2(g)
Cl2(aq)
B. C(s) + H2O(l)
CO(g) + H2(g)
C2H5OH(l) + 3O2
C. 2CO2(g) + 3H2O(g)
D. Na2CO3(s) + HCl (aq)
2NaCl (aq) + CO2(g) + H2O(l)
∆H = -25 kJ
∆H = +131kJ
∆H = +1239kJ
∆H = -28kJ
9. Consider the following equilibrium:
H2 (g) + I2(g)
2HI(g)
Which graph represents what happens when some HI is removed and a new equilibrium
is established?
10. Consider the following equilibrium:
CO(g) + H2O(g)
CO2(g) + H2(g)
What will cause a shift in the equilibrium?
A. adding a catalyst
B. changing volume
C. adding an inert gas
D. changing temperature
11. The equilibrium expression for a reaction is
[H+]6
Keq = ------------------[Bi3+]2[H2S]3
The reaction could be
A. 6H+ + BiS(s)
B. 6H+ (aq) + Bi2S3 (s)
C. 2Bi 3+ (aq) + 3H2S (aq)
D. 2Bi 3+ (aq) + 3H2S (aq)
2Bi 3+ (aq) + 3H2S(g)
2Bi 3+ (aq) + 3H2S(g)
Bi2S3(s) + 6H+(aq)
Bi2S3 (aq) + 6H+ (aq)
∆H = -41kJ
12. Consider the following equilibrium:
Co(H2O)6 2+ (aq) + 4ClCoCl42- (aq) + 6H2O(l)
(pink)
(blue)
When the temperature is increased, the solution turns a dark blue. Based on this
observation, the reaction is
A. exothermic and the Keq has increased.
B. exothermic and the Keq has decreased.
C. endothermic and the Keq has increased.
D. endothermic and the Keq has decreased.
13. Consider the following equilibrium:
2O3(g)
3O2(g)
Keq = 36
What is the concentration of O3 when the equilibrium concentration
Of O2 is 6.0 X 10-2 mol/L?
A. 2.4 X 10-3 mol/L
B. 4.0 X 10-2 mol/L
C. 6.0 X 10-2 mo/L
D. 9.0 X 10-2 mol/L
August 2000
7. Which of the following does not apply to all chemical equilibrium systems?
A. They are closed.
B. The macroscopic properties are constant.
C. Forward and reverse reaction rates are equal.
D. There are equal concentrations of reactants and products.
8. Consider the following equilibrium:
2NOCl(g)
2NO (g) + Cl2(g)
A flask is filled with NOCl, NO and Cl2. Initially there was a total of 5.0 moles of
gases present. When equilibrium is reached, there is a total of 6.0 moles of gases present.
Which of the following explains this observation?
A. The reaction proceeded left because the Trial Keq > Keq
B. The reaction proceeded left because the Trial Keq < Keq
C. The reaction proceeded right because the Trial Keq > Keq
D. The reaction proceeded right because the Trial Keq < Keq
9. Consider the following reaction:
C3H8 (g) + 5O2(g) 3CO2(g) + 4H2O(g)
Which of the following applies to the forward reaction?
A.
B.
C.
D.
Entropy
increases
increases
decreases
decreases
∆H = -2202kJ
Enthalpy
increases
decreases
increases
decreases
10. Consider the following equilibrium:
2NO2(g)
N2O4 (g) + energy
The number of moles of NO2 at equilibrium could be increased by
A. adding N2O4
B. adding a catalyst.
C. decreasing the temperature.
D. decreasing the volume by increasing the pressure.
11. What is the Keq expression for
Sb3+ (aq) + Cl-(aq) + H2O(l)
12. Consider the following equilibrium:
H2 (g) + I2(g)
2HI(g)
What is the value Keq for the reaction rewritten as:
2HI (g)
H2(g) + I2(g)
A. –50.0
B. 0.0200
C. 25.0
D. 50.0
SbOCl (s) + 2H+ (aq)
Keq = 50.0
Keq = ?
13. Consider the following equilibrium:
2NO2(g)
N2O4 (g)
Keq = 1.15
The equilibrium concentration of NO2 is 0.50 mol/L. Calculate the equilibrium
Concentration of N2O4 (g).
A. 0.22 mol/L
B. 0.29 mol/L
C. 0.43 mol/L
D. 0.58 mol/L
January 2001
7. All chemical equilibriums have:
I.
II.
III.
rates that are continuing to change
an equilibrium constant expression
equal concentrations of products and reactants
A. II only
B. III only
C. I and II only
D. I and III only
8. From the following, select the situation where both enthalpy and entropy favour
the reaction toward products:
A.
B.
C.
D.
Enthalpy
increasing
increasing
decreasing
decreasing
Entropy
increasing
decreasing
decreasing
increasing
9. Consider the following equilibrium:
2NO(g) + Br2(g)
2NOBr(g) + energy
The equilibrium will shift to the left as a result of
A. adding a catalyst.
B. adding some NO (g).
C. increasing the volume.
D. decreasing the temperature.
10. Consider the following equilibrium:
PCl3(g) + 3NH3(g)
P(NH2)3 (g) + 3HCl(g)
The volume of the equilibrium system is increased and a new equilibrium is established.
How have the rates been affected?
A.
B.
C.
D.
Rate (forward)
increased
decreased
decreased
did not change
Rate (reverse)
decreased
increased
decreased
did not change
11. Starting with equal moles of reactants, which of the following equilibrium systems
most favours the reactants?
A. SO2(g) + NO2(g)
B. CO(g) + H2O(g)
C. H2(g) + I2(g)
D. N2 (g) + O2(g)
SO3 (g) + NO(g)
CO2(g) + H2(g)
2HI(g)
2NO(g)
Keq= 3.4
Keq= 31.4
Keq= 10
Keq= 1.0X10-31
12. Consider the following equilibrium reaction:
N2O4(g)
2NO2(g)
At time t1, heat is applied to the system. Which of the following best describes the
equilibrium reaction and the change in Keq?
A. exothermic and Keq increases
B. exothermic and Keq decreases
C. endothermic and Keq increases
D. endothermic and Keq decreases
13. Consider the following:
PCl3(g) + Cl2(g)
PCl5(g)
Keq = 0.45 at 227°C
Initially, a 1.00L flask is filled with 0.100mol PCl3, 0.100mol Cl2, and 0.100mol PCl5
at 227°C. Use KTrial to predict the change in [Cl2] as equilibrium is established.
April 2001
7. Consider the following equilibrium reaction:
2ICl(g)
I2(g) + Cl2(g)
Some ICl is added to an empty flask. How do the reaction rates change as
the system approaches equilibrium?
A.
B.
C.
D.
Forward rate
increases
increases
decreases
decreases
Reverse rate
increases
decreases
increases
decreases
8. In an equilibrium system, continuing microscopic changes indicate that the equilibrium
is
A. dynamic.
B. complete.
C. exothermic.
D. spontaneous.
9. Consider the following equilibrium:
4CuO(s) + energy
2Cu2O(s) + O2(g)
The equilibrium will shift to the right as a result of
A. adding CuO (s).
B. removing O2 (g).
C. adding a catalyst.
D. decreasing the temperature.
10. Consider the following equilibrium:
N2(g) + 3H2(g)
2NH3(g)
The volume of the system is decreased. The equilibrium shifts
A. left since the reverse rate is greater than the forward rate.
B. left since the forward rate is greater than the reverse rate.
C. right since the reverse rate is greater than the forward rate.
D. right since the forward rate is greater than the reverse rate.
11. Consider the following equilibrium:
2SO3(g)
2SO2(g) + O2(g)
∆Η = +198kJ
When the temperature is increased, the equilibrium will shift
A. left with Keq becoming larger.
B. right with Keq becoming larger.
C. left with Keq becoming smaller.
D. right with Keq becoming smaller.
12. Starting with equal concentrations of reactants, which of the following will be
closest to completion at equilibrium?
A. CO(g) + Cl2(g)
B. PCl3(g) + Cl2(g)
C. CO(g) + Cl2(g)
D. CH3O2 (g) + NO2(g)
COCl2(g)
PCl5(g)
COCl2(g)
CH3O2NO2(g)
Keq=22
Keq= 2.9 X 10-2
Keq=4.5 X 10 –9
Keq=2.1 X 10 -12
13. Consider the following equilibrium:
2COF2(g)
CO2(g) + CF4(g)
At equilibrium, a 1.00L container contains 7.07 X 10-4 mol COF2, 1.00 X 10-3 mol CO2,
and 1.00 X 10-3 mol CF4. What is the value of Keq?
A. 7.07 X 10-4
B. 1.41 X 10-3
C. 0.500
D. 2.00
June 2001
7. Consider the following reaction:
2ICl(g)
I2(g) + Cl2(g)
A closed container is initially filled with ICl (g). What are the changes in the
rate of the forward reaction and [I2], as the system approaches equilibrium?
8. The entropy of a system is a term used to describe
A. randomness.
B. heat content.
C. average kinetic energy.
D. stored chemical energy.
9. Consider the following equilibrium:
Cu2+ (aq) + 4Br-(aq) + energy
Blue
colourless
CuBr4 2-(aq)
green
Which of the following will cause this equilibrium to change from blue to green?
A. adding NaBr (s)
B. adding NaNO3 (s)
C. adding a catalyst
D. decreasing the temperature
10. Consider the following equilibrium:
Ni(s) + 4CO(g)
Ni(CO)2(l)
∆Η =−160.8kJ
Which of the following will cause this equilibrium to shift to the left?
A. add some CO
B. decrease the volume
C. remove some Ni(CO)4
D. increase the temperature
11. Consider the following equilibrium:
N2O4(g) + energy
2NO2(g)
Which of the following shows the relationship between concentration and time
as a result of adding a catalyst at time t = 1?
12. Consider the following equilibrium:
H2S(g) + I2(g)
2HI(g) + S(s)
What is the equilibrium expression for this reaction?
[HI]2
A Keq=--------------[H2S]
[H2S]
B. Keq=--------------[HI]2
[HI]2[S]
C. Keq=--------------[H2S]P[I2]
[H2S]P[I2]
D. Keq=--------------[HI]2[S]
13. Consider the following equilibrium:
CO(g) + H2O(g)
CO2(g) + H2(g)
Keq = 5.0
At equilibrium, the [CO]= 0.20mol/L, [H2O]= 0.30mol/L, and [H2]= 0.90mol/L.
Calculate the equilibrium [CO2].
A. 0.013 mol/L
B. 0.066 mol/L
C. 0.33 mol/L
D. 1.0mol/L
14. Consider the following:
CO2(g) + CF4(g)
2COF2(g)
In a reaction container the initial concentrations are:
[CO2]= 0.50mol/L, [CF4]= 0.50mol/L, [COF2]= 0.30 mol/L
Keq= 0.50
To reach equilibrium, the reaction will proceed
A. left since Trial Keq < K eq
B. left since Trial Keq > K eq
C. right since Trial Keq < K eq
D. right since Trial Keq > K eq
August 2001
7. All chemical equilibriums must have
A. Keq = 1
B. [reactants]=[products].
C. rate forward = rate reverse.
D. mass of reactants = mass of products.
8. Consider the following equilibrium reaction:
4HCl(g) + O2(g)
2H2O(g) + 2Cl2(g) + 111.4kJ
For the forward reaction, how do enthalpy and entropy change?
A.
B.
C.
D.
Enthalpy
increases
decreases
increases
decreases
Entropy
decreases
decreases
increases
increases
9. Consider the following equilibrium:
CH3Cl(aq) + OH- (aq)
CH3OH(aq) + Cl-(aq)
The equilibrium will shift to the left as a result of the addition of
A. HNO3
B. KNO3
C. NaOH
D. CH3Cl
10. Consider the following equilibrium at 25°C :
Ni(s) + 4CO(g)
Ni(CO)4(l)
For this reaction
A. Keq = [CO]4
1
B. Keq= -------------[CO]4
[Ni(CO)4(l)]
C. Keq= ---------------[CO]4 [Ni]
[Ni(CO)4(l)]
D. Keq= ---------------[CO]4
11. Consider the following equilibrium:
2COF2(g)
CO2(g) + CF4(g)
Keq=2.00
At equilibrium, [CO2]=0.050mol/L and [CF4]=0.050mol/L. What t is [COF2] at
equilibrium?
A. 0.0012 mol/L
B. 0.035 mol/L
C. 0.050 mol/L
D. 0.22 mol/L
12. Consider the following equilibrium:
H2O(g) + Cl2O(g)
2HOCl(g)
Keq= 0.0900
Initially, a 1.00L flask is filled with 0.100mol of H2O, 0.100mol of Cl2O and 0.100mol of
HOCl. As equilibrium is established, the reaction proceeds to the
A. left because KTrial > K eq
B. left because KTrial < K eq
C. right because KTrial > K eq
D. right because KTrial < K eq
January 2002
7. Consider the following:
2SO2(g) + O2(g)
2SO3(g)
Initially, SO3 is added to an empty flask. How do the rate of the forward reaction and
[SO3] change as the system proceeds to equilibrium?
8. Consider the following reaction:
2NH3(g) + energy
N2(g) + 3H2(g)
What positions do minimum enthalpy and maximum entropy tend toward?
Use the following equilibrium equation to answer questions 9 and 10.
CO2(g) + H2(g)
H2O(g) + CO(g)
9. Which two stresses will each cause the equilibrium to shift to the left?
A. increase [H2] , increase [CO]
B. decrease [H2] , increase [H2O]
C. increase [CO2] , decrease [CO]
D. decrease [CO2] , decrease [H2O]
10. Which of the following graphs represents the forward rate of reaction when H2O(g) is
added to the above equilibrium at time t = 1 ?
11. Consider the following:
2NH3 (g)
N2(g) + 3H2(g)
Initially, some NH3 is placed into a 1.0L container. At equilibrium there is 0.030mol N2
present. What is the [H2] at this equilibrium?
A. 0.010 mol/L
B. 0.030 mol/L
C. 0.060 mol/L
D. 0.090 mol/L
12. Which reaction has the following equilibrium expression?
[NO2]4[H2O]6
Keq=----------------[NH3]4[O2]7
A. 4NH3(g) + 7O2(g)
B. 4NH3(aq) + 7O2(g)
C. 4NO2(aq) + 6H2O(l)
D. 4NO2(g) + 6H2O(g)
4NO2(g) + 6H2O(g)
4NO2(aq) + 6H2O(l)
4NH3(g) + 7O2(g)
4NH3(g) + 7O2(g)
13. What will cause the Keq for an exothermic reaction to increase?
A. increasing [reactants]
B. decreasing [products]
C. increasing the temperature
D. decreasing the temperature
April 2002
7. Consider the following:
H2(g) + I2(g)
2HI(g)
Initially, HI is added to an empty flask. How do the rates of the forward and reverse
reactions change as the system proceeds to equilibrium?
8. Consider the following reaction:
2H2O(l) + energy 2H2 (g) + O2(g)
Determine the enthalpy and entropy changes for the above reaction?
Use the following equilibrium equation to answer questions 9 and 10.
2CO(g) + O2(g)
2CO2(g) + energy
9. Which of the following two stresses will each cause the system to shift to the right?
A. increase temperature, increase volume
B. decrease temperature, increase volume
C. increase temperature, decrease volume
D. decrease temperature, decrease volume
10. Which of the following shows the forward rate of reaction when the temperature of
the system is increased at time t = 1 ?
11. Consider the following:
2SO2(g) + O2(g)
2SO3(g)
Initially, 0.030mol SO2 and 0.030mol O2 are placed into a 1.0L container. At equilibrium,
there is 0.020 mol O2 present. What is the [SO2] at equilibrium?
A. 0.010 mol/L
B. 0.020 mol/L
C. 0.030 mol/L
D. 0.040 mol/L
12. What is the equilibrium expression for the following system?
CaCO3(s) + 2HF(g)
CaF2(s) + H2O(g) + CO2(g)
[HF]2
A. Keq=-------------------[H2O][CO2]
[H2O][CO2]
C. Keq= --------------[CaCO3][HF]2
[H2O][CO2]
B. Keq=---------------[HF]2
[CaF2] [H2O][CO2]
D. Keq= ---------------------[CaCO3][HF]2
13. What will cause the Keq for an endothermic reaction to decrease?
A. adding a catalyst
B. increasing the surface area
C. increasing the temperature
D. decreasing the temperature
Answer Key
Jan 99
7
8
9
10
11
12
13
C
B
C
A
D
C
C
Apr 99
7
8
9
10
11
12
13
Jan 00
7
8
9
10
11
12
13
A
C
A
C
B
C
B
A
D
C
C
D
C
A
7
8
9
10
11
12
13
D
D
B
C
D
A
D
D
C
B
B
B
D
C
7
8
9
10
11
12
13
C
A
B
D
B
A
D
Apr 02
7
8
9
10
11
12
13
B
C
D
B
A
B
D
C
C
C
A
D
A
B
Aug 99
7
8
9
10
11
12
13
Jun 00
7
8
9
10
11
12
13
Apr 01
Jan 02
7
8
9
10
11
12
13
7
8
9
10
11
12
13
Apr 00
Jan 01
7
8
9
10
11
12
13
D
C
C
A
A
D
D
Jun 99
B
C
B
D
C
C
A
Aug 00
7
8
9
10
11
12
13
Jun 01
7
8
9
10
11
12
13
14
A
A
A
D
C
A
C
C
A
A
C
A
A
B
A
D
D
B
A
A
B
B
Aug 01
7
8
9
10
11
12
C
B
A
B
B
A