Chapter 19, Problem 19.112QP

(a)

Interpretation Introduction

Interpretation:

The equilibrium constant of given cell should be calculated and concentration of ${\text{Fe}}^{\text{2+}}$ ion should be calculated, when equal volume of $\text{0}\text{.75M}$ solutions of ${\text{Fe}}^{\text{2+}}$ and ${\text{Ag}}^{\text{+}}$ are mixed.

Concept introduction:

Nernst equation:

The relationship between standard cell potential and cell potential at non-standard conditions and the reaction quotient are given by Nernst equation it is,

${\text{E}}_{\text{cell}}\text{=}{\text{E°}}_{\text{cell}}\text{-}\frac{\text{2}\text{.303}\text{RT}}{\text{nF}}\text{logQ}$

Where,

$\begin{array}{l}{\text{E}}_{\text{cell}}\text{ is}\text{cell potential}\\ {\text{E°}}_{\text{cell}}\text{is}\text{standard cell potential}\\ \text{R}\text{is}\text{gas}\text{constant}\\ \text{T}\text{is}\text{temperature}\\ \text{Q}\text{is}\text{reaction quotient}\end{array}$

(b)

Interpretation Introduction

Interpretation:

The equilibrium constant of given cell should be calculated and concentration of ${\text{Fe}}^{\text{2+}}$ ion should be calculated, when equal volume of $\text{0}\text{.75M}$ solutions of ${\text{Fe}}^{\text{2+}}$ and ${\text{Ag}}^{\text{+}}$ are mixed.

Concept introduction:

Nernst equation:

The relationship between standard cell potential and cell potential at non-standard conditions and the reaction quotient are given by Nernst equation it is,

${\text{E}}_{\text{cell}}\text{=}{\text{E°}}_{\text{cell}}\text{-}\frac{\text{2}\text{.303}\text{RT}}{\text{nF}}\text{logQ}$

Where,

$\begin{array}{l}{\text{E}}_{\text{cell}}\text{ is}\text{cell potential}\\ {\text{E°}}_{\text{cell}}\text{is}\text{standard cell potential}\\ \text{R}\text{is}\text{gas}\text{constant}\\ \text{T}\text{is}\text{temperature}\\ \text{Q}\text{is}\text{reaction quotient}\end{array}$