Chapter 19, Problem 19.153MP

Interpretation Introduction

(a)

Interpretation:

A balanced equation for the cell reaction should be written and the cell potential at 25⁰ C should be calculated.

Concept introduction:

The Nernst equation allows to calculate cell potential at non-standard conditions.

$E=E^0-\frac{0.0592\text{ V}}{n}\log Q$

Here,

E − non-standard cell potential

E⁰ − standard cell potential

n − number of electrons passed through the cell

Q − reaction quotient

Interpretation Introduction

(b)

Interpretation:

The cell potential at 25⁰ C after the precipitation of $\text{AgBr}$ should be calculated. A balanced equation for the cell reaction under these conditions should be written.

Concept introduction:

The Nernst equation allows to calculate cell potential at non-standard conditions.

$E=E^0-\frac{0.0592\text{ V}}{n}\log Q$

Here,

E − non-standard cell potential

E⁰ − standard cell potential

n − number of electrons passed through the cell

Q − reaction quotient

Interpretation Introduction

(c)

Interpretation:

The standard reduction potential for the half cell reaction $\text{AgBr(s) + e }\to \text{ Ag(s) }+{\text{ Br}}^{-}\text{(aq)}$ should be calculated.

Concept introduction:

The standard cell potential of overall reaction is given by the sum of the standard half-cell potentials for oxidation and reduction.

${\text{E}}_{overall}^0={\text{E}}_{ox}^0+{\text{ E}}_{red}^0$