Chapter 18, Problem 18.9P

Interpretation Introduction

Interpretation:

The amount of copper added in 1000 mL of water to produce electrode potential of +0.32 V needs to be calculated.

Concept Introduction:

Electrode potential can be calculated by the Nernst equation,

  $E_{cell}=E^0{}_{cell}-\frac{RT}{nF}\ln Q$

Where,

  $E_{cell}$ =cell potential at non-standard state.

  $E^0{}_{cell}$ = cell potential at standard state.

R = universal gas constant = 8.314

T = temperature

F = faradays constant

n = number of moles of electrons

Q = reaction quotient

Copper content in the cell can be calculated by Nernst equation

  $E=E^0+\frac{0.0592}{n}\log (\frac{x}{C_{ion}})$

Where,

E = electrode potential

  $C_{ion}$ = metal concentration

n = charge on metallic ion

  $E^0$ = standard electrode potential

x = copper content