Chapter 22, Problem 22.87SP

Interpretation Introduction

Interpretation:

The time in hours which are required to produce 10 kg of magnesium and the volume in litres of chlorine obtained at STP are to be determined.

Concept introduction:

• Faraday’s 1^st law of electricity states that the amount of substance produced at an electrode is proportional to the amount of electricity utilized to produce the substance. Mathematically, $\text{w = Z}\times \text{I}\times \text{t}$ where w is the amount of substance produced, $\text{Z}$ is the electrochemical equivalent, $\text{I}$is the current utilized in ampere and t is the time in seconds for which the current flows.
• Electrochemical equivalent is the amount of substance produced when 1 A current is passed through the solution for 1 sec.
• $\text{1A}\text{s = 1 Faraday = 96500 C}$
• $\text{Z=}\frac{\text{Atomic}\text{mass}}{\text{n × 96500}}$, where n is the number of electrons exchanged.
• One mole of an ideal gas occupies 22.4 L volume at STP.

Given:

Amount of magnesium produced= $\text{10}\text{kg}$

Amount of electricity passed = ${\text{1 × 10}}^{\text{4}}\text{ A}$