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For the equilibrium A+B=C+D K was measured to be 1.20 at 25 °C and 1.15 x 10² at 300 °C. What is AH° for the reaction?

For the equilibrium A+B=C+D K was measured to be 1.20 at 25 °C and 1.15 x 10² at 300 °C. What is AH° for the reaction?

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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**Equilibrium Constant and Enthalpy Change** For the equilibrium reaction: \[ \text{A} + \text{B} \rightleftharpoons \text{C} + \text{D} \] The equilibrium constant (\( K \)) was measured to be 1.20 at 25 °C and \( 1.15 \times 10^{-2} \) at 300 °C. Determine \( \Delta H^\circ \) for the reaction. --- **Understanding the Reaction Parameters:** - **Equilibrium Constant (\( K \))**: This value indicates the ratio of the concentration of products to reactants at equilibrium. A larger \( K \) favors products, while a smaller \( K \) favors reactants. - **Temperature Influence on \( K \)**: Changes in temperature can shift the equilibrium position, affecting \( K \). In this scenario, observe how \( K \) changes from a higher value at a lower temperature to a significantly smaller value at a higher temperature. - **Enthalpy Change (\( \Delta H^\circ \))**: This is the heat absorbed or released during a reaction at constant pressure. It can be determined using the van 't Hoff equation, which relates the change in \( K \) over temperature to \( \Delta H^\circ \).
Transcribed Image Text:**Equilibrium Constant and Enthalpy Change** For the equilibrium reaction: \[ \text{A} + \text{B} \rightleftharpoons \text{C} + \text{D} \] The equilibrium constant (\( K \)) was measured to be 1.20 at 25 °C and \( 1.15 \times 10^{-2} \) at 300 °C. Determine \( \Delta H^\circ \) for the reaction. --- **Understanding the Reaction Parameters:** - **Equilibrium Constant (\( K \))**: This value indicates the ratio of the concentration of products to reactants at equilibrium. A larger \( K \) favors products, while a smaller \( K \) favors reactants. - **Temperature Influence on \( K \)**: Changes in temperature can shift the equilibrium position, affecting \( K \). In this scenario, observe how \( K \) changes from a higher value at a lower temperature to a significantly smaller value at a higher temperature. - **Enthalpy Change (\( \Delta H^\circ \))**: This is the heat absorbed or released during a reaction at constant pressure. It can be determined using the van 't Hoff equation, which relates the change in \( K \) over temperature to \( \Delta H^\circ \).
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