For the reaction 2A(g) + B(s) C(g) + D(g) at 700 °C Kc = 0.692 0.310 moles of A and 0.310 moles of B are placed in a 1.00-L closed container, heated to 700 °C and allowed to reach equilibrium. What is the concentration of C once equilibrium is established? 0.0900 M (Your answer) 0.194 M 0.141 M 0.0704 M 0.0968 M (Correct answer)
For the reaction 2A(g) + B(s) C(g) + D(g) at 700 °C Kc = 0.692 0.310 moles of A and 0.310 moles of B are placed in a 1.00-L closed container, heated to 700 °C and allowed to reach equilibrium. What is the concentration of C once equilibrium is established? 0.0900 M (Your answer) 0.194 M 0.141 M 0.0704 M 0.0968 M (Correct answer)
Chemistry
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Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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Chapter1: Chemical Foundations
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![For the reaction
\[ 2A(g) + B(s) \rightleftharpoons C(g) + D(g) \]
at 700 °C, the equilibrium constant \( K_C \) is 0.692.
0.310 moles of A and 0.310 moles of B are placed in a 1.00-L closed container, heated to 700 °C and allowed to reach equilibrium. What is the concentration of C once equilibrium is established?
- 0.0900 M (Your answer)
- 0.194 M
- 0.141 M
- 0.0704 M
- 0.0968 M (Correct answer)](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F6d7773ea-2418-45b6-94fc-b17f139a153f%2F0e6f8012-c57f-41ce-af45-b0e1ec0f3d78%2Fkyjq8cyd_processed.jpeg&w=3840&q=75)
Transcribed Image Text:For the reaction
\[ 2A(g) + B(s) \rightleftharpoons C(g) + D(g) \]
at 700 °C, the equilibrium constant \( K_C \) is 0.692.
0.310 moles of A and 0.310 moles of B are placed in a 1.00-L closed container, heated to 700 °C and allowed to reach equilibrium. What is the concentration of C once equilibrium is established?
- 0.0900 M (Your answer)
- 0.194 M
- 0.141 M
- 0.0704 M
- 0.0968 M (Correct answer)
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