Chapter 6, Problem 6M.1AST

(a)

Interpretation Introduction

Interpretation:

The standard cell potential has to be calculated.

Concept Introduction:

Standard potential ${\text{E}}^{\text{o}}$ is the measure of the electron pulling power that occurs in the electrode of a chemical reaction.  In a galvanic cell, the electrons are pulled in opposite directions in each electrode.

Standard cell potential ${\text{E}}^{\text{o}}{}_{\text{cell}}$ is the difference between the standard potentials of the two electrodes.  The formula to calculate the standard cell potential is,

  ${\text{E}}^{\text{o}}{}_{\text{cell}}{\text{=E}}^{\text{o}}{}_{\left(\text{reduction}\right)}{\text{-E}}^{\text{o}}{}_{\left(\text{oxidation}\right)}$

Reduction happens in the cathode (right hand electrode) and oxidation takes place in the anode (left hand electrode).

(b)

Interpretation Introduction

Interpretation:

The net ionic equation for the cell reaction has to be written.

(c)

Interpretation Introduction

Interpretation:

The strongest reducing agent has to be given.