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2 A(g) = B(g) + 3 C(g) For the above chemical reaction, a mixture of 4.40 moles of A, 2.49 moles of B, and 3.64 moles of C are placed in a 3-L container at a specified temperature. Assuming the system is allowed to reach equilibrium and the temperature stayed the same, the equilibrium amount of A was found to be 2.34 moles. What is the equilibrium constant, Kc, for this chemical reaction? Round your final answer to two decimal places.

2 A(g) = B(g) + 3 C(g) For the above chemical reaction, a mixture of 4.40 moles of A, 2.49 moles of B, and 3.64 moles of C are placed in a 3-L container at a specified temperature. Assuming the system is allowed to reach equilibrium and the temperature stayed the same, the equilibrium amount of A was found to be 2.34 moles. What is the equilibrium constant, Kc, for this chemical reaction? Round your final answer to two decimal places.

Chemistry
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
Chapter1: Chemical Foundations
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2 A(g) = B(g) + 3 C(g) For the above chemical reaction, a mixture of 4.40 moles of A, 2.49 moles of B, and 3.64 moles of C are placed in a 3-L container at a specified temperature. Assuming the system is allowed to reach equilibrium and the temperature stayed the same, the equilibrium amount of A was found to be 2.34 moles. What is the equilibrium constant, Kc, for this chemical reaction? Round your final answer to two decimal places.
Transcribed Image Text:2 A(g) = B(g) + 3 C(g) For the above chemical reaction, a mixture of 4.40 moles of A, 2.49 moles of B, and 3.64 moles of C are placed in a 3-L container at a specified temperature. Assuming the system is allowed to reach equilibrium and the temperature stayed the same, the equilibrium amount of A was found to be 2.34 moles. What is the equilibrium constant, Kc, for this chemical reaction? Round your final answer to two decimal places.
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