Chapter 19, Problem 19.162MP

Interpretation Introduction

(a)

Interpretation:

Standard electrode potential of the ordinary alkaline battery should be calculated.

Concept introduction:

Standard reduction potential of a cell can be calculated with the following equation.

$E_{cell}^0=E_{cathode}^0-E_{anode}^0$

Here, $E_{cell}^0$ - Standard electrode potential of the cell (Battery)

$E_{cathode}^0$ - Standard electrode potential of the cathode

$E_{anode}^0$ - Standard electrode potential of the anode

Interpretation Introduction

(b)

Interpretation:

Cathode reaction of the super-iron battery should be stated.

Concept introduction:

In the cathode of a battery, the reduction reaction take place. In the reduction process gain of electron/s takes place. The oxidation state of the atom increases.

Interpretation Introduction

(c)

Interpretation:

The number of Coulombs of charge released by reduction of FeO_{42 -to Fe(OH)3& reduction of MnO2 to MnO(OH) should be compared.}

Concept introduction:

An electron released by any element or ion carries a charge of 1.60×10-19 Coulombs.