   Chapter 19.6, Problem 19.8CYU

Chapter
Section
Textbook Problem

The following reaction has an E° value of −0.76 V:H2(g) + Zn2+(aq) → Zn(s) + 2 H+(aq)Calculate ΔrG° for this reaction. Is the reaction product- or reactant-favored at equilibrium?

Interpretation Introduction

Interpretation:

The ΔrGo for the following reaction has to be determined and find whether it is reactant favoured or product favoured.

H2(g) + Zn2+(aq) Zn(s) + 2H+(aq)

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 sysytem 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

Explanation

The given reaction is as follows.

H2(g) + Zn2+(aq) Zn(s) + 2H+(aq)

Let’s calculate the ΔG0 for the reaction.

ΔG0= -nFE0n = 2F = 96485C/mol  E0= -0

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