Chapter 5, Problem 5.79P

Interpretation Introduction

Interpretation:

Standard reaction enthalpy and entropy for the given cell should be determined within the given temperature range where ${\text{E}}_{cell}^{\Theta }\text{ at 293 K = 1}\text{.2335 V}$ and ${\text{E}}_{cell}^{\Theta }\text{ at 303 K = 1}\text{.2251 V}$.

Concept introduction:

Standard Gibbs energy is calculated as below,

  ${\text{Δ}}_r{\text{G}}^{\Theta }\text{= }\text{}-\nu {\text{FE}}_{cell}^{\Theta }\boxed{\begin{array}{c}\text{F = Faraday's constant}\\ \nu \text{ = No}\text{. of electrons transferred}\\ {\text{E}}_{cell}^{\Theta }\text{ = Standard cell potential at temperature, T}\end{array}}$

Standard entropy of reaction is determined as follows,

${\Delta }_r{S}^{\Theta }\text{ = }\frac{\nu F\left(E_{cell}^{\Theta }-E_{cell}^{\Theta }\text{'}\right)}{T-T\text{'}}\boxed{\begin{array}{c}\text{F = Faraday's constant}\\ \nu \text{ = No}\text{. of electrons transferred}\\ {\text{E}}_{cell}^{\Theta }\text{ = Standard cell potential at temperature, T}\\ E_{cell}^{\Theta }\text{'}\text{ = Standard cell potential at temperature, T}\text{'}\end{array}}$

Standard reaction enthalpy can be calculated using the given formula,

${\Delta }_r{H}^{\Theta }\text{ = }{\Delta }_r{G}^{\Theta }\text{ + T}{\Delta }_r{S}^{\Theta }\boxed{\begin{array}{c}{\Delta }_r{H}^{\Theta }\text{ = }S\tan dardreactionenthalpy\\ {\Delta }_r{S}^{\Theta }\text{ = }S\tan dardentropyofreaction\\ {\Delta }_r{G}^{\Theta }\text{ = Standard Gibbs energy}\end{array}}$