Chapter 18, Problem 18.45QP

Interpretation Introduction

Interpretation:

To calculate the amount of magnesium deposited during the electrolysis reaction.

Concept introduction:

In an electrolysis process the supply of electrons will reduce the Mg²⁺ ion in to magnesium the half-cell reaction can be written as follows

$\text{Cathode (Reduction)}{\text{Mg}}^{{}_{\text{2+}}}{}_{\text{(aq)}}{\text{+ 2e}}^{\text{-}}\stackrel{}{\to }{\text{Mg}}_{\text{(s)}}$

In the above reaction two electrons reduces Mg²⁺ into magnesium metal.

One Faraday represents the one mole of electrons, from knowing the number of moles of electron needed to reduce one mole of magnesium ions; we can determine the number of moles of magnesium produced by the following equation. Further from the number of moles of magnesium calculated, mass of magnesium produced can be determines.

$\begin{array}{l}\text{Number}\text{of}\text{mole}\text{of}\text{Mg=Farady×}\frac{\text{1}\text{mole}\text{of}\text{Mg}}{\text{2mole}\text{of}{\text{e}}^{\text{-}}}\\ \text{Mass}\text{=}\text{Number}\text{of}\text{mole}\text{of}\text{Mg×Atomic}\text{mass}\text{of}\text{Mg}\end{array}$

To find: The mass of magnesium produced during electrolytic process.