1.
Equilibrium Problem Set #2
For each of the following reactions, describe what effect and increase in pressure
would have on the equilibrium position of the reaction (i.e. shift right, shift left, no
change)
a. 2H2S(g) <===> 2H2 (g) + S2 (g)
LEFT
b. 2N2O5(g) <===> 4NO2 (g) + O2 (g) LEFT
c. 4NO(g) + 2O2 (g) <===> 2N2O4(g) RIGHT
d. 2NO(g) + Br2 (g) <===> 2NOBr(g) RIGHT
e. CO(g) + 2H2 (g) <===>CH3OH(g)
RIGHT
f. SO2 (g) + NO2 (g) <===>SO3(g) + NO(g) NO CHANGE
2. In which direction would the equilibrium shift for the equation in 1a if S2 were removed
from the reaction vessel?
RIGHT
3. In which direction would the equilibrium shift for the equation in 1b if N 2O5 were
added?
RIGHT
4. In which direction would the equilibrium shift for the equation in 1c if O 2 were
removed?
LEFT
5. In which direction would the equilibrium shift for the equation in 1d if pressure were
decreased?
LEFT
6. In which direction would the equilibrium shift for the equation in 1e if CH 3OH were
removed?
RIGHT
7. In which direction would the equilibrium shift for the equation in 1f if heat were added?
(the rxn is endothermic).
RIGHT
8. What would be the effect on the equilibrium position of an equilibrium mixture of Br 2,
F2, and BrF5 if the total pressure of the system were decreased?
2BrF5(g) <===> Br2(g) + 5F2 (g)
RIGHT
9. What would be the effect on the equilibrium position of an equilibrium mixture of
carbon, oxygen, and carbon monoxide if the total pressure of the system were
decreased?
2C2 (s) +O2 (g) <===> 2CO(g)
RIGHT
10. A weather indicator can be made with a hydrate of cobalt (II) chloride, which changes
color as a result of the following reaction:
[Co(H2O) 6] Cl2 (s) <===> [Co(H2O) 6] Cl2 (s) +2H20(g)
pink
blue
Does a pink color indicate “moist” or “dry” air? Explain.
Moist --- when water is added the equilibrium would shift left, making a higher
equilibrium concentration of the pink compound
11. Consider the reaction:
CaCO3(s) <===> CaO(s) + CO2 (g)
Will the mass of CaCO3 at equilibrium increase, decrease or remain the same if
(a) CO2 is added to the equilibrium system? INCREASE
(b) the pressure is increased? INCREASE
(c) solid CaO is removed? DECREASE
12. The reaction between NO and O2 is exothermic.
2NO(g) + O2 (g) <===> 2NO2 (g)
Will the concentration of NO2 at equilibrium increase, decrease, or remain the same if
(a) additional O2is introduced? INCREASE
(b) additional NO is introduced? INCREASE
(c) the total pressure is decreased? DECREASE
(d) the temperature is increased? DECREASE
13. Predict whether the equilibrium for the photosynthesis reaction described by the
equation:
6CO2 (g) + 6H20(ℓ)<===> C6H12O6(s) + 6O2 (g)
H° = 2801.69 kJ/mol
would shift to the right, shift to the left, or remain unchanged if
(a) [CO2] were increased; RIGHT
(b) PO2 were increased; NO CHANGE
(c) one half of the C6H12O6 were removed; RIGHT
(d) the total pressure were decreased; NO CHANGE
(e) the temperature were decreased; LEFT
(f) a catalyst were added. NO CHANGE
14. What would be the effect of increasing the temperature on each of the following
systems at equilibrium?
a. H2 (g) + I2 (g) <===> 2HI(g) + 9.45 kJ LEFT
b. PCl5(g) + 92.5 kJ <===> PCl 3(g) + Cl2 (g) RIGHT
c. 2SO2 (g) + O2 (g) <===> 2SO3(g); H° = -198 kJ/mol LEFT
d. 2NOCl(g) <===> 2NO(g) + Cl2 (g); H° = 75 kJ/mol RIGHT
e. C(s) + H2O(g) + 131 kJ <===> CO(g) + H2 (g) RIGHT
15. What would be the effect of increasing the pressure by decreasing the volume on each
of the following systems at equilibrium?
a. 2CO(g) + O2 (g) <===> 2CO2 (g) RIGHT
b. 2NO(g) <===> N2 (g) + O2 (g) NO CHANGE
c. N2O4(g) <===> 2NO2 (g) LEFT
d. Ni(s) + 4CO(g) <===> Ni(CO) 4(g) RIGHT
e. N2 (g) + 3H2 (g) <===> 2NH3(g) RIGHT
16. The value of Kc is 0.020 at 2870° for the reaction shown below. There are 0.800 mole
of N2, 0.500 mole of O2, and 0.400 mole of NO in a 1.00-liter container at 2870°C. Is
the system at equilibrium or must the forward or reverse action occur to a greater
extent to bring the system to equilibrium?
N2 (g) + O2 (g) <===> 2NO(g)
(.400)2
 .400
(.800)(.500)
Q  Keq
Q
 not at equilibrium - - - reverse rxn will predominat e until equilibrium is reached
17. Given: A(g) + B(g) <===> C(g) + D(g)
At equilibrium a 1.00-liter container was found to contain 1.60 mole of C, 1.60 mol of D,
0.40 mol of A, and 0.40 mole of B. Calculate the equilibrium constant for this reaction.
Keq 
(1.60)(1.60)
 16
(0.40)(0.40)