Chapter 15.3, Problem 15.29QAP

Interpretation Introduction

(a)

Interpretation:

Write the half- reactions and the overall cell reaction for the given voltaic cell

  $\text{Pb}(s)|{\text{Pb}}^{2+}(aq)||{\text{Cu}}^{2+}(aq)|\text{Cu}(s)$

Concept Introduction:

The shorthand notation of a cell reaction indicates phase boundary by a single vertical line $\text{(}|)$ and salt bridge is denotes by a double vertical line $\text{(}\left|\right|)$ . In this notation on the left side of salt bridge oxidation reaction which occurred at anode and on the right side of salt bridge; reduction reaction which occurred at cathode. The electrodes are written on the extreme corners; anode on extreme left and cathode on extreme right. The reactants in each half-cell are always first, followed by the products.

For the positive standard cell potential, the reaction is spontaneous in nature and for negative value it is non-spontaneous.

Interpretation Introduction

(b)

Interpretation:

Write the half- reactions and the overall cell reaction for the given voltaic cell

  $\text{Cr(}s)|{\text{Cr}}^{2+}(aq)\left|\right|{\text{Ag}}^{+}(aq)|\text{Ag(}s)$

Concept Introduction:

The shorthand notation of a cell reaction indicates phase boundary by a single vertical line $\text{(}|)$ and salt bridge is denotes by a double vertical line $\text{(}\left|\right|)$ . In this notation on the left side of salt bridge oxidation reaction which occurred at anode and on the right side of salt bridge; reduction reaction which occurred at cathode. The electrodes are written on the extreme corners; anode on extreme left and cathode on extreme right. The reactants in each half-cell are always first, followed by the products.

If the standard cell potential is positive, then the reaction is spontaneous and if the standard cell potential is negative, then the reaction is non-spontaneous