Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter13: Chemical Equilibrium
Section: Chapter Questions
Problem 117CP: A mixture of N2, H2, and NH3 is at equilibrium [according to the equationN2(g)+3H2(g)2NH3(g)] as...
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![### Determining the Equilibrium Constant \( K_c \) for a Modified Reaction
#### Given Reaction:
\[ 2H_2S(g) \rightleftharpoons 2H_2(g) + S_2(g) \qquad K_c = 0.0160 \]
#### Question:
What is the value of \( K_c \) for the reaction below?
\[ 4H_2(g) + 2S_2(g) \rightleftharpoons 4H_2S(g) \]
#### Solution:
When manipulating equilibrium expressions, it's essential to understand how changes in coefficients and direction of the reaction affect the equilibrium constant.
Here, the original reaction is:
\[ 2H_2S(g) \rightleftharpoons 2H_2(g) + S_2(g) \quad K_c = 0.0160 \]
To obtain the new reaction:
\[ 4H_2(g) + 2S_2(g) \rightleftharpoons 4H_2S(g) \]
we notice that it is the reverse reaction of the original one and the coefficients are doubled.
For the reverse reaction:
\[ K'_c = \frac{1}{K_c} \]
Doubling the coefficients of all substances in the reaction changes the equilibrium constant as follows:
\[ K''_c = \left( K'_c \right)^2 \]
#### Calculation:
1. First, reverse the original reaction:
\[ K'_c = \frac{1}{0.0160} \]
2. Calculate \( K'_c \):
\[ K'_c = 62.5 \]
3. Since the coefficients are doubled in the new reaction:
\[ K''_c = \left( 62.5 \right)^2 \]
\[ K''_c = 3906.25 \]
Thus, the equilibrium constant \( K_c \) for the new reaction is:
\[ K''_c = 3906.25 \]
#### Answer:
\[ K''_c = \boxed{3906.25} \]
For the user to input this value, there is an input box labeled "Kc of new reaction" and an "Enter" button next to it to submit their answer.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fa9c8a3ef-f821-4363-8862-d3250243b3b2%2F20b93e69-d853-43a3-a034-62c47e2a16b4%2F191h0sg_processed.jpeg&w=3840&q=75)
Transcribed Image Text:### Determining the Equilibrium Constant \( K_c \) for a Modified Reaction
#### Given Reaction:
\[ 2H_2S(g) \rightleftharpoons 2H_2(g) + S_2(g) \qquad K_c = 0.0160 \]
#### Question:
What is the value of \( K_c \) for the reaction below?
\[ 4H_2(g) + 2S_2(g) \rightleftharpoons 4H_2S(g) \]
#### Solution:
When manipulating equilibrium expressions, it's essential to understand how changes in coefficients and direction of the reaction affect the equilibrium constant.
Here, the original reaction is:
\[ 2H_2S(g) \rightleftharpoons 2H_2(g) + S_2(g) \quad K_c = 0.0160 \]
To obtain the new reaction:
\[ 4H_2(g) + 2S_2(g) \rightleftharpoons 4H_2S(g) \]
we notice that it is the reverse reaction of the original one and the coefficients are doubled.
For the reverse reaction:
\[ K'_c = \frac{1}{K_c} \]
Doubling the coefficients of all substances in the reaction changes the equilibrium constant as follows:
\[ K''_c = \left( K'_c \right)^2 \]
#### Calculation:
1. First, reverse the original reaction:
\[ K'_c = \frac{1}{0.0160} \]
2. Calculate \( K'_c \):
\[ K'_c = 62.5 \]
3. Since the coefficients are doubled in the new reaction:
\[ K''_c = \left( 62.5 \right)^2 \]
\[ K''_c = 3906.25 \]
Thus, the equilibrium constant \( K_c \) for the new reaction is:
\[ K''_c = 3906.25 \]
#### Answer:
\[ K''_c = \boxed{3906.25} \]
For the user to input this value, there is an input box labeled "Kc of new reaction" and an "Enter" button next to it to submit their answer.
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