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Untitled - Kelly Walsh High School

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Chemical Equilibria 217<br />

10. Write K p expression for each of the following equilibria.<br />

a. 2 NO 2(g) K N 2(g) 2 O 2(g)<br />

b. C(s) H 2O(g) K CO(g) H 2(g)<br />

c. 2 Zn(s) O 2(g) K 2 ZnO(s)<br />

d. 2 C 4H 10(g) 13 O 2(g) K 8 CO 2(g) 10 H 2O(l)<br />

e. MnCO 3(s) K CO 2(g) MnO(s)<br />

11. Calculate K p for the following equilibrium at 523 K:<br />

NH 2COONH 4(s) K 2 NH 3(g) CO 2(g)<br />

At this temperature K c 1.58 10 8 .<br />

12. Nitrogen oxide, NO, reacts with hydrogen gas, H 2, to establish the following<br />

equilibrium:<br />

2 NO(g) 2 H 2(g) K N 2(g) 2 H 2O(g)<br />

The following concentrations of materials are sealed in a container: 0.250<br />

M NO, 0.100 M H 2, and 0.200 M H 2O. Construct an ICE table for K c.<br />

13. The following equilibrium is established at 500 K:<br />

S 2(g) C(s) K CS 2(g).<br />

The initial pressure of sulfur vapor was 0.431 atm. Construct an ICE table<br />

for K p.<br />

14. Indicate how the partial pressure of hydrogen will change if the following<br />

stresses are applied to the equilibrium below:<br />

H 2(g) CO 2(g) K H 2O(l) CO(g) H 41 kJ<br />

a. Adding carbon dioxide b. Adding water<br />

c. Adding a catalyst d. Increasing the temperature<br />

e. Increasing the pressure<br />

15. Determine K c for the following equilibrium:<br />

2 CH 4(g) K C 2H 2(g) 3 H 2(g)<br />

In order to determine this value, a mixture initially 0.0300 M in CH 4 was<br />

allowed to come to equilibrium. At equilibrium, the concentration of C 2H 2<br />

was 0.01375 M.<br />

16. The compound PH 3BCl 3 decomposes on heating by the following equilibrium:<br />

PH 3BCl 3(s) K PH 3(g) BCl 3(g) K p 1.60<br />

Determine the equilibrium partial pressures of the gases resulting when a<br />

sample of PH 3BCl 3 is placed in a sealed flask and allowed to come to equilibrium.<br />

17. Hydrogen sulfide gas decomposes at 700°C according to the following equilibrium:<br />

2 H 2S(g) K 2 H 2(g) S 2(g)<br />

At this temperature, K c for this reaction is 9.1 10 8 , what will be the equilibrium<br />

concentrations of the gases if the initial concentration of H 2S was<br />

0.200 M H 2S?

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