Chapter 11, Problem 17E

(a)

Interpretation Introduction

Interpretation: The oxidizing agent and the reducing agent needs to be identified and the direction of electron flow needs to be explained.

Concept Introduction: Oxidizing agent accepts and electron and get reduced, i.e., it oxidizes other substances

Reducing agent loses an electron and get oxidized, i.e., it reduces other substances.

Standard cell potential is the potential of a cell under standard condition, with taken as 1 M conc., Pressure= 1 atm, temperature= ${\text{25}}^{\text{0}}\text{C}$

(b)

Interpretation Introduction

Interpretation: The standard cell potential needs to be determined.

Concept Introduction :

Standard reduction potential measures the tendency of a chemical substance or species to get reduced. It can be defined relative to the Standard hydrogen potential reference electrode, with a given potential of 0.00 V.

Standard cell potential is the potential of a cell under standard condition, with taken as 1 M conc., Pressure= 1 atm, temperature= ${\text{25}}^{\text{0}}\text{C}$

(c)

Interpretation Introduction

Interpretation: The electrodes which increases and decreases in mass as the reaction proceeds needs to be determined.

Concept Introduction : Anodes are cathodes are called electrodes. Copper bar and zinc bar are immersed in a ${\text{CuSO}}_{\text{4}}$ solution and ${\text{ZnSO}}_{\text{4}}$ solution respectively. The zinc and copper bar are called electrodes. In the galvanic cell, oxidation takes place in anode and reduction takes place in the cathode. The oxidation and reduction at the electrodes are as follows:

At Zinc electrode (anode)

  $\text{Zn (s) }\to {\text{Zn}}^{+2}(aq)+2e^{-}$

At Copper electrode (cathode)

  ${\text{Cu}}^{+2}(aq)+2e^{-}\to \text{Cu}\text{(s)}$