   Chapter 20, Problem 88CWP

Chapter
Section
Textbook Problem

# Molten CaC12 is electrolyzed for 8.00 h to produce Ca(s) and Cl2(g).a. What current is needed to produce 5.52 kg of calcium metal?b. If 5.52 kg calcium metal is produced, what mass (in kg) of C12 is produced?

(a)

Interpretation Introduction

Interpretation: The time taken for the electrolysis of CaCl2 and the mass of calcium metal produced is given. The amount of current produced and the mass of chlorine produced is to be calculated.

Concept introduction: The number of atoms is calculated as,

Numberofatoms=Mass×6.022×1023Atomicmass

The current flowing through the cell is calculated by the formula,

Current=ChargeTime

To determine: The current produced by the electrolysis of CaCl2 .

Explanation

Given

The time taken for electrolysis is 8h=2.88×104s .

The mass of calcium metal produced is 5.52kg=5.52×103g .

The oxidation half cell reaction for the electrolysis of CaCl2 is,

2ClCl2(g)+2e

The reduction half cell reaction for the electrolysis of CaCl2 is,

Ca++2eCa(s)

The net cell reaction for the electrolysis of CaCl2 is,

CaCl2Ca(s)+Cl2(g)

Thus, the production of one atom of calcium metal causes the transport of two electrons.

The atomic mass of calcium is 40.078g/mol .

The number of atoms of calcium metal produced is calculated as,

Numberofatoms=Mass×6.022×1023Atomicmass

Substitute the value of mass and atomic mass of calcium in the above formula.

Numberofatoms=5.52×103g×6

(b)

Interpretation Introduction

Interpretation: The time taken for the electrolysis of CaCl2 and the mass of calcium metal produced is given. The amount of current produced and the mass of chlorine produced is to be calculated.

Concept introduction: The number of atoms is calculated as,

Numberofatoms=Mass×6.022×1023Atomicmass

The current flowing through the cell is calculated by the formula,

Current=ChargeTime

To determine: The mass of chlorine gas produced in the electrolysis of CaCl2 .

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