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C. Consider a chemical reaction. At a temperature T, = 300. K and an external pressure P, the enthalpy of reaction is A, H (T,, P) = 400.J and the Gibbs potential of reaction is A, G(T,,P) = 100. J. %3D We will prove later that Gibbs-Helmholtz relation can also extended to describe chemical reactions ((), ArH Assuming this relation to hold true, consider the following: ƏT T2

C. Consider a chemical reaction. At a temperature T, = 300. K and an external pressure P, the enthalpy of reaction is A, H (T,, P) = 400.J and the Gibbs potential of reaction is A, G(T,,P) = 100. J. %3D We will prove later that Gibbs-Helmholtz relation can also extended to describe chemical reactions ((), ArH Assuming this relation to hold true, consider the following: ƏT T2

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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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Assuming that deltarH s independent of temperature, determine deltarG(T2,P) for T2= 400K

C. 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 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:
Transcribed Image Text:C. 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 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:
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