Chapter 15.3, Problem 32PP

(a)

Interpretation Introduction

Interpretation:

Describe the overall and half-cell reactions of the given voltaic cell reaction and also write the shorthand notation.

  ${\text{Mn(s) +Sn}}^{\text{2+}}\text{(aq)}\to {\text{Mn}}^{\text{2+}}\text{(aq)+ Sn(s)}$

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.

(b)

Interpretation Introduction

Interpretation:

Describe the overall and half-cell reactions of the given voltaic cell reaction and also write the shorthand notation.

  ${\text{Ni(s) +2Ag}}^{\text{+}}\text{(aq)}\to {\text{Ni}}^{\text{2+}}\text{(aq)+2Ag(s)}$

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.