C. Consider a chemical reaction. At a temperature T1 = 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. 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: T
C. Consider a chemical reaction. At a temperature T1 = 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. 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: T
Introduction to Chemical Engineering Thermodynamics
8th Edition
ISBN:9781259696527
Author:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart
Publisher:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart
Chapter1: Introduction
Section: Chapter Questions
Problem 1.1P
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Assuming that deltarH is independent of temperature, estimate the temperature at which the forward reaction is favorable.
![### Thermodynamic Concepts in Chemical Reactions
**Consideration of a Chemical Reaction:**
At a temperature \( T_1 = 300.\,\text{K} \) and an external pressure \( P \), the enthalpy of reaction is given by:
\[ \Delta_r H(T_1, P) = 400.\,\text{J} \]
Additionally, the Gibbs potential of the reaction is:
\[ \Delta_r G(T_1, P) = 100.\,\text{J} \]
**Extension of Gibbs-Helmholtz Relation:**
We will prove later that the Gibbs-Helmholtz relation can also be extended to describe chemical reactions. The relation is expressed as:
\[
\left( \frac{\partial}{\partial T} \left( \frac{\Delta_r G}{T} \right) \right)_P = -\frac{\Delta_r H}{T^2}
\]
Assuming this relation to hold true, we can make further considerations.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F37df213a-2c14-4822-a979-37f159717cfc%2F47fd5731-4b70-46d8-bcd0-8e60606831fb%2Fsi2k2mu_processed.png&w=3840&q=75)
Transcribed Image Text:### Thermodynamic Concepts in Chemical Reactions
**Consideration of a Chemical Reaction:**
At a temperature \( T_1 = 300.\,\text{K} \) and an external pressure \( P \), the enthalpy of reaction is given by:
\[ \Delta_r H(T_1, P) = 400.\,\text{J} \]
Additionally, the Gibbs potential of the reaction is:
\[ \Delta_r G(T_1, P) = 100.\,\text{J} \]
**Extension of Gibbs-Helmholtz Relation:**
We will prove later that the Gibbs-Helmholtz relation can also be extended to describe chemical reactions. The relation is expressed as:
\[
\left( \frac{\partial}{\partial T} \left( \frac{\Delta_r G}{T} \right) \right)_P = -\frac{\Delta_r H}{T^2}
\]
Assuming this relation to hold true, we can make further considerations.
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