Untitled - Kelly Walsh High School

Chemical Equilibria 217
10. Write K p expression for each of the following equilibria.
a. 2 NO 2(g) K N 2(g) 2 O 2(g)
b. C(s) H 2O(g) K CO(g) H 2(g)
c. 2 Zn(s) O 2(g) K 2 ZnO(s)
d. 2 C 4H 10(g) 13 O 2(g) K 8 CO 2(g) 10 H 2O(l)
e. MnCO 3(s) K CO 2(g) MnO(s)
11. Calculate K p for the following equilibrium at 523 K:
NH 2COONH 4(s) K 2 NH 3(g) CO 2(g)
At this temperature K c 1.58 10 8 .
12. Nitrogen oxide, NO, reacts with hydrogen gas, H 2, to establish the following
equilibrium:
2 NO(g) 2 H 2(g) K N 2(g) 2 H 2O(g)
The following concentrations of materials are sealed in a container: 0.250
M NO, 0.100 M H 2, and 0.200 M H 2O. Construct an ICE table for K c.
13. The following equilibrium is established at 500 K:
S 2(g) C(s) K CS 2(g).
The initial pressure of sulfur vapor was 0.431 atm. Construct an ICE table
for K p.
14. Indicate how the partial pressure of hydrogen will change if the following
stresses are applied to the equilibrium below:
H 2(g) CO 2(g) K H 2O(l) CO(g) H 41 kJ
a. Adding carbon dioxide b. Adding water
c. Adding a catalyst d. Increasing the temperature
e. Increasing the pressure
15. Determine K c for the following equilibrium:
2 CH 4(g) K C 2H 2(g) 3 H 2(g)
In order to determine this value, a mixture initially 0.0300 M in CH 4 was
allowed to come to equilibrium. At equilibrium, the concentration of C 2H 2
was 0.01375 M.
16. The compound PH 3BCl 3 decomposes on heating by the following equilibrium:
PH 3BCl 3(s) K PH 3(g) BCl 3(g) K p 1.60
Determine the equilibrium partial pressures of the gases resulting when a
sample of PH 3BCl 3 is placed in a sealed flask and allowed to come to equilibrium.
17. Hydrogen sulfide gas decomposes at 700°C according to the following equilibrium:
2 H 2S(g) K 2 H 2(g) S 2(g)
At this temperature, K c for this reaction is 9.1 10 8 , what will be the equilibrium
concentrations of the gases if the initial concentration of H 2S was
0.200 M H 2S?