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Liquid methanol, CH;OH(1), is an important solvent in industry and can also be used as a fuel. Methanol may be synthesized in the gas state from carbon monoxide gas, CO(g), and hydrogen gas, H,(g), in a chemical reaction system that comes to equilibrium in a closed vessel at 225 °C. (a) Write the balanced chemical equation for the formation of methanol gas from carbon monoxide gas and hydrogen gas at 225 °C. (b) The equilibrium constant, K, for this reaction at 225 °C is 6.3 × 10¯³. Predict the relative concentration of the methanol gas when equilibrium is established. (c) Based on your answer for (b), predict whether this equilibrium system could generate large quantities of methanol. Explain your answer. (d) What would be the equilibrium constant for the reverse reaction?

Liquid methanol, CH;OH(1), is an important solvent in industry and can also be used as a fuel. Methanol may be synthesized in the gas state from carbon monoxide gas, CO(g), and hydrogen gas, H,(g), in a chemical reaction system that comes to equilibrium in a closed vessel at 225 °C. (a) Write the balanced chemical equation for the formation of methanol gas from carbon monoxide gas and hydrogen gas at 225 °C. (b) The equilibrium constant, K, for this reaction at 225 °C is 6.3 × 10¯³. Predict the relative concentration of the methanol gas when equilibrium is established. (c) Based on your answer for (b), predict whether this equilibrium system could generate large quantities of methanol. Explain your answer. (d) What would be the equilibrium constant for the reverse reaction?

Chemistry: The Molecular Science
Chemistry: The Molecular Science
5th Edition
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter12: Chemical Equilibrium
Section: Chapter Questions
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3. Liquid methanol, CH;OH(1), is an important solvent in industry and can also be used as a fuel. Methanol may be synthesized in the gas state from carbon monoxide gas, CO(g), and hydrogen gas, H2(g), in a chemical reaction system that comes to equilibrium in a closed vessel at 225 °C. (a) Write the balanced chemical equation for the formation of methanol gas from carbon monoxide gas and hydrogen gas at 225 °C. (b) The equilibrium constant, K, for this reaction at 225 °C is 6.3 × 10¬³. Predict the relative concentration of the methanol gas when equilibrium is established. (c) Based on your answer for (b), predict whether this equilibrium system could generate large quantities of methanol. Explain your answer. (d) What would be the equilibrium constant for the reverse reaction?
Transcribed Image Text:3. Liquid methanol, CH;OH(1), is an important solvent in industry and can also be used as a fuel. Methanol may be synthesized in the gas state from carbon monoxide gas, CO(g), and hydrogen gas, H2(g), in a chemical reaction system that comes to equilibrium in a closed vessel at 225 °C. (a) Write the balanced chemical equation for the formation of methanol gas from carbon monoxide gas and hydrogen gas at 225 °C. (b) The equilibrium constant, K, for this reaction at 225 °C is 6.3 × 10¬³. Predict the relative concentration of the methanol gas when equilibrium is established. (c) Based on your answer for (b), predict whether this equilibrium system could generate large quantities of methanol. Explain your answer. (d) What would be the equilibrium constant for the reverse reaction?
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