Chapter 14.1, Problem 1TY

Interpretation Introduction

Interpretation:

The number of moles of tin ion required to reduce it by one coulomb charge has to be calculated.

Concept introduction:

Electric charge:

Electric charge is defined as magnitude of charge of a mole of electron $\left(\text{1}{\text{.602×10}}^{\text{-19}}\text{C}\right)\left(\text{6}{\text{.022×10}}^{\text{23}}{\text{mol}}^{\text{-1}}\right)\text{=9}{\text{.649×10}}^{\text{14}}\text{C}$.  It is expressed in terms of coulombs (C).  $\text{9}{\text{.649×10}}^{\text{14}}\text{C}$ is Faraday constant.

The electric charge in coulombs can be expressed as,

$\text{q=n}\text{.N}\text{.F}$

Where q = coulombs

n = unit charges per molecule

N = moles

F= $\frac{\text{Coulombs}}{\text{mole}{\text{e}}^{\text{-}}}$