Chapter 19, Problem 19.80QP

Interpretation Introduction

Interpretation:

The amount of magnesium present at the end of the reaction and molar concentration of ${\text{Ag}}^{+}$ and ${\text{Mg}}^{2+}$ at the equilibrium conditions has to be found.

Concept Introduction:

The standard electrode potential of a cell${\text{(E}}^{°}{}_{\text{cell}})$ is the difference in electrode potential of the cathode and anode.

  ${\text{E}}^{\text{°}}{}_{\text{cell}}={\text{E}}^{\text{°}}{}_{\text{cathode}}-{\text{E}}^{\text{°}}{}_{\text{anode}}$

The relation between electrode potential and equilibrium constant: cell potential and equilibrium constant are related by the given equation.

  ${\text{E}}^{°}{}_{\text{cell}}\text{=}\frac{\text{RT}}{\text{nF}}\text{lnK}$

Where,

  ${\text{E}}^{°}{}_{\text{cell}}$ is the standard electrode potential

  $\text{n}$ is the number of electrons

  $\text{K}$ is the formation constant

  $\text{R}$ is the universal gas constant $\text{(R=8}{\text{.314JK}}^{\text{-1}}{\text{mol}}^{\text{-1}})$

  $\text{T}$ is the temperature

  $\text{F}$ is the Faraday constant $\text{(F=9}\text{.64853399}\times {\text{10}}^4{\text{Cmol}}^{\text{-1}})$

Mole is the mass of the substance that is having Avogadro number of particles.  The number of moles of a given substance can be calculated by multiplying its volume with concentration.

Molar concentration or molarity is the ratio of number of moles of solute to the volume of the solution in litre.