Hydrogen and carbon dioxide gases react at a high temperature to give water and carbon monoxide: H2(g) + CO2(g) H2O(g) + CO(g)Laboratory measurements at 986°C show that there are 0.11 mol each of CO(g) and H2O(g), and 0.087 mol each of H2(g) and CO2(g) at equilibrium in a 1.00 L container. Calculate the equilibrium constant for the reaction at 986°C.Suppose 0.050 mol each of H2(g) and CO2(g) are placed in a 2.00 L container. When equilibrium is achieved at 986°C, what amounts of CO(g) and H2O(g), in moles, would be present?

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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

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Hydrogen and carbon dioxide gases react at a high temperature to give water and carbon monoxide: H₂(g) + CO₂(g) H₂O(g) + CO(g)
1. Laboratory measurements at 986°C show that there are 0.11 mol each of CO(g) and H₂O(g), and 0.087 mol each of H₂(g) and CO₂(g) at equilibrium in a 1.00 L container. Calculate the equilibrium constant for the reaction at 986°C.
2. Suppose 0.050 mol each of H₂(g) and CO₂(g) are placed in a 2.00 L container. When equilibrium is achieved at 986°C, what amounts of CO(g) and H₂O(g), in moles, would be present?

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