Chemistry 102, Test Chapter 13-14 Worksheet With Answers - 1997 Page 10
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1123.(22)At 1500 K, the equilibrium constant for the reaction
2 SO
(g) + O
(g)
2 SO
(g)
2
2
3
is 0.15. The equilibrium constant for the reaction
2 SO
(g)
2 SO
+ O
(g)
at the same temperature is
3
2
2
3
1. 6.7
2. 0.51
3. 2.3 x 10
4. 4.5
Answer: 1. 6.7
2
(P
)
↔ 2SO
SO3
2SO
(g) + O
(g)
(g)
K =
= 0.15
2
2
3
(P
)(P
)
SO2
O2
2
(P
)
(P
)
1
(g) ↔ 2SO
SO2
O2
2SO
(g) + O
(g)
K =
=
= 6.7
3
2
2
2
(P
)
0.15
SO3
The second reaction is just the first reaction written backwards. The two equilibrium
constant expressions are reciprocals of each other. K for the second reaction is the
reciprocal of K for the first reaction.
24.(16 Consider the reaction
3 O
(g)
2 O
(g)
2
3
What is the relationship between Kp and Kc?
2
1. Kp = Kc
2. Kp = Kc (RT)
3. Kp = Kc (RT)
-1
-2
4. Kp = Kc (RT)
5. Kp = Kc (RT)
-1
Answer: 4. Kp = Kc(RT)
Kp and Kc are both equilibrium constants but with different units. Kp uses Pressure units
(atm) for the equilibrium amounts and Kc uses concentration in molarity [ ] for the
equilibrium amounts. The two are related by the equation
∆n
where ∆n = # of product gas moles - # of reactant gas moles
Kp = Kc(RT)
for this reaction ∆n = 2-3 = -1
since there are 2 moles of gaseous products and 3 moles of
gaseous reactants.
25.(24)For an exothermic reaction
A + B
C + D + heat
an increase in temperature will
1. increase the rate and shift the equilibrium to the right.
2. increase the rate and shift the equilibrium to the left.
3. decrease the rate and shift the equilibrium to the right.
4. decrease the rate and shift the equilibrium to the left.
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