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C. Consider a chemical reaction. At a temperature T1 enthalpy of reaction is A,H(T,, P) = 400. J and the Gibbs potential of reaction is A, G(T,,P) 100.J. 300. K and an external pressure P, the

C. Consider a chemical reaction. At a temperature T1 enthalpy of reaction is A,H(T,, P) = 400. J and the Gibbs potential of reaction is A, G(T,,P) 100.J. 300. K and an external pressure P, the

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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Is the reaction endothermic or exothermic? Is the forward or backward reaction favorable under these conditions? 

**Chemical Reactions and Thermodynamics** **Consider a chemical reaction.** At a temperature \( T_1 = 300. \, \text{K} \) and an external pressure \( P \), the enthalpy of reaction is \( \Delta_r H(T_1, P) = 400. \, \text{J} \) and the Gibbs potential of reaction is \( \Delta_r G(T_1, P) = 100. \, \text{J} \). We will prove later that the Gibbs-Helmholtz relation can also be extended to describe chemical reactions: \[ \left( \frac{\partial}{\partial T} \left( \frac{\Delta_r G}{T} \right) \right)_P = -\frac{\Delta_r H}{T^2}. \] Assuming this relation to hold true, consider the following: --- **Explanation of the Gibbs-Helmholtz Relation in Chemical Reactions:** The Gibbs-Helmholtz equation connects changes in temperature to changes in Gibbs energy divided by temperature, under constant pressure. It provides an approach to quantify how the Gibbs free energy of a reaction varies with temperature, taking the enthalpy change into account. This is important for understanding the temperature dependence of reaction spontaneity.
Transcribed Image Text:**Chemical Reactions and Thermodynamics** **Consider a chemical reaction.** At a temperature \( T_1 = 300. \, \text{K} \) and an external pressure \( P \), the enthalpy of reaction is \( \Delta_r H(T_1, P) = 400. \, \text{J} \) and the Gibbs potential of reaction is \( \Delta_r G(T_1, P) = 100. \, \text{J} \). We will prove later that the Gibbs-Helmholtz relation can also be extended to describe chemical reactions: \[ \left( \frac{\partial}{\partial T} \left( \frac{\Delta_r G}{T} \right) \right)_P = -\frac{\Delta_r H}{T^2}. \] Assuming this relation to hold true, consider the following: --- **Explanation of the Gibbs-Helmholtz Relation in Chemical Reactions:** The Gibbs-Helmholtz equation connects changes in temperature to changes in Gibbs energy divided by temperature, under constant pressure. It provides an approach to quantify how the Gibbs free energy of a reaction varies with temperature, taking the enthalpy change into account. This is important for understanding the temperature dependence of reaction spontaneity.
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By studying the temperature, enthalpy, and Gibbs free energy we can conclude that if the reaction is exothermic or endothermic and forward or backward in nature. 

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