The Δ r G o for the following reaction has to be determined and find whether it is reactant favoured or product favoured. H 2 (g) + Zn 2+ (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 - W ΔU = Change in internal energy Q = Heat added to the system W=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. ΔG 0 = -nFE 0 n = Number of moles transferred per mole of reactant and products F = Faradayconstant=96485C/mol E 0 = Volts = Work(J)/Charge(C) The relation between standard cell potential and equilibrium constant is as follows. lnK = nE 0 0 .0257 at 298K

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Chapter 19.6, Problem 1CYU

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.

$lnK = nE00.0257 at 298K$

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