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42 Consider the following reaction at equilibrium: 2H2(g)+52(g)=2H25(g)+heat 00000000 In a 10.0-L container, an equilibrium mixture contains 2.06 g of H2, 11.1 g of $2 and 69.0 g of H25. If a 4.00-L container has an equilibrium mixture of 0.320 mol of H2 and 2.45 mol of H2S, what is the [S2] if temperature remains constant?

42 Consider the following reaction at equilibrium: 2H2(g)+52(g)=2H25(g)+heat 00000000 In a 10.0-L container, an equilibrium mixture contains 2.06 g of H2, 11.1 g of $2 and 69.0 g of H25. If a 4.00-L container has an equilibrium mixture of 0.320 mol of H2 and 2.45 mol of H2S, what is the [S2] if temperature remains constant?

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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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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42 Consider the following reaction at equilibrium: 2H2(g)+52(g)=2H25(g)+heat 00000000 In a 10.0-L container, an equilibrium mixture contains 2.06 g of H2, 11.1 g of $2 and 69.0 g of H25. If a 4.00-L container has an equilibrium mixture of 0.320 mol of H2 and 2.45 mol of H2S, what is the [S2] if temperature remains constant?
Transcribed Image Text:42 Consider the following reaction at equilibrium: 2H2(g)+52(g)=2H25(g)+heat 00000000 In a 10.0-L container, an equilibrium mixture contains 2.06 g of H2, 11.1 g of $2 and 69.0 g of H25. If a 4.00-L container has an equilibrium mixture of 0.320 mol of H2 and 2.45 mol of H2S, what is the [S2] if temperature remains constant?
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