Consider a reaction in which two compounds, A and B, react to form a single product, C. The reaction is known to be exothermic. Initially, a stoichiometric mixture of A and B is heated in a closed container. As the reaction proceeds, the temperature of the system increases. However, when the reaction reaches equilibrium, the temperature of the system remains constant. Explain this observation and provide a theoretical explanation for why the temperature stops increasing at equilibrium.
Consider a reaction in which two compounds, A and B, react to form a single product, C. The reaction is known to be exothermic. Initially, a stoichiometric mixture of A and B is heated in a closed container. As the reaction proceeds, the temperature of the system increases. However, when the reaction reaches equilibrium, the temperature of the system remains constant. Explain this observation and provide a theoretical explanation for why the temperature stops increasing at equilibrium.
World of Chemistry, 3rd edition
3rd Edition
ISBN:9781133109655
Author:Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCoste
Chapter17: Equilibrium
Section: Chapter Questions
Problem 31A
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Consider a reaction in which two compounds, A and B, react to form a single product, C. The reaction is known to be exothermic. Initially, a stoichiometric mixture of A and B is heated in a closed container. As the reaction proceeds, the temperature of the system increases. However, when the reaction reaches equilibrium, the temperature of the system remains constant.
Explain this observation and provide a theoretical explanation for why the temperature stops increasing at equilibrium.
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