Chapter 19, Problem 19.36CP

Interpretation Introduction

(a)

Interpretation:

Whether the cell voltage increase, decrease or remain the same when $5.0{\text{ M CuSO}}_4$ is added to the cathode compartment should be explained.

Concept introduction:

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

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

E − non-standard cell potential

E⁰ − standard cell potential

n − number of electrons passed through the cell

Q − reaction quotient

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

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

Interpretation Introduction

(b)

Interpretation:

Whether the cell voltage increase, decrease or remain the same when $5.0{\text{ M H}}_2{\text{SO}}_4$ is added to the cathode compartment should be explained.

Concept introduction:

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

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

E − non-standard cell potential

E⁰ − standard cell potential

n − number of electrons passed through the cell

Q − reaction quotient

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

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

Interpretation Introduction

(c)

Interpretation:

Whether the cell voltage increase, decrease or remain the same when $5.0\text{ M Zn}\left({\text{NO}}_3\right)$ is added to the anode compartment should be explained.

Concept introduction:

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

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

E − non-standard cell potential

E⁰ − standard cell potential

n − number of electrons passed through the cell

Q − reaction quotient

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

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

Interpretation Introduction

(d)

Interpretation:

Whether the cell voltage increase, decrease or remain the same when $1.0\text{ M Zn}\left({\text{NO}}_3\right)$ is added to the anode compartment should be explained.

Concept introduction:

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

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

E − non-standard cell potential

E⁰ − standard cell potential

n − number of electrons passed through the cell

Q − reaction quotient

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

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