   Chapter 19, Problem 71GQ

Chapter
Section
Textbook Problem

The standard potential, E°, for the reaction of Zn(s) and Cl2(g) is +2.12 V. What is the standard free energy change, ΔrG°, for the reaction?

Interpretation Introduction

Interpretation:

The standard free energy for the given reaction by using E0 has to be determined.

Concept introduction:

According to the first law of thermodynamics, the change in internal energy of a system is equal ti the heat added to the system minus the work done by the system.

The equation is as follows.

ΔU = Q - WΔU = Change in internal energyQ = Heat added to the systemW=Work done by the system

In voltaic cell, the maximum cell potential is directly related to the free energy difference between the reactants and products in the cell.

ΔG0= -nFE0n = Number of moles transferred per mole of reactant and productsF = Faradayconstant=96485C/mol  E0= Volts = Work(J)/Charge(C)

The relation between standard cell potential and equilibrium constant is as follows.

lnK = nE00.0257 at 298K

The relation between solubility product Ksp and equilibrium constant is as follows.

Ksp= e+lnK

The relation between the standard free energy and standard free energy is as follows.

ΔG0= -nE0F

Explanation

The reaction between Zn and Cl2 is as follows.

Zn + Cl2 ZnCl2

Number of electrons transferred = 2e-

E0 value of the Zn and Cl2 is 2

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