Molten CaC1 2 is electrolyzed for 8.00 h to produce Ca( s ) and Cl 2 ( 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 C1 2 is produced?

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(a) Interpretation Introduction Interpretation: The time taken for the electrolysis of CaCl 2 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, Number of atoms = Mass × 6.022 × 10 23 Atomic mass The current flowing through the cell is calculated by the formula, Current = Charge Time To determine: The current produced by the electrolysis of CaCl 2 . Explanation Given The time taken for electrolysis is 8 h = 2.88 × 10 4 s . The mass of calcium metal produced is 5.52 kg = 5.52 × 10 3 g . The oxidation half cell reaction for the electrolysis of CaCl 2 is, 2Cl − → Cl 2 ( g ) + 2 e − The reduction half cell reaction for the electrolysis of CaCl 2 is, Ca + + 2 e − → Ca ( s ) The net cell reaction for the electrolysis of CaCl 2 is, CaCl 2 → Ca ( s ) + Cl 2 ( g ) Thus, the production of one atom of calcium metal causes the transport of two electrons. The atomic mass of calcium is 40.078 g / mol . The number of atoms of calcium metal produced is calculated as, Number of atoms = Mass × 6.022 × 10 23 Atomic mass Substitute the value of mass and atomic mass of calcium in the above formula. Number of atoms = 5.52 × 10 3 g × 6 (b) Interpretation Introduction Interpretation: The time taken for the electrolysis of CaCl 2 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, Number of atoms = Mass × 6.022 × 10 23 Atomic mass The current flowing through the cell is calculated by the formula, Current = Charge Time To determine: The mass of chlorine gas produced in the electrolysis of CaCl 2 .

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Chemistry: An Atoms First Approach

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Chemistry: An Atoms First Approach

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Steven S. Zumdahl + 1 other

Publisher: Cengage Learning

ISBN: 9781305079243

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(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,

Number of atoms=Mass×6.022×1023Atomic mass

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

Current=ChargeTime

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

Explanation of Solution

Given

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

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

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

2Cl−→Cl2(g)+2e−

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

Ca++2e−→Ca(s)

The net cell reaction for the electrolysis of CaCl2 is,

CaCl2→Ca(s)+Cl2(g)

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

The atomic mass of calcium is 40.078 g/mol .

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

Number of atoms=Mass×6.022×1023Atomic mass

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

Number of atoms=5.52×103 g×6

Answer 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,

Number of atoms=Mass×6.022×1023Atomic mass

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 .

Molten CaC1 2 is electrolyzed for 8.00 h to produce Ca( s ) and Cl 2 ( 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 C1 2 is produced?

Chemistry: An Atoms First Approach

Solutions

Chemistry: An Atoms First Approach

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?

Explanation of Solution

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Molten CaC1 2 is electrolyzed for 8.00 h to produce Ca( s ) and Cl 2 ( 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 C1 2 is produced?

Chemistry: An Atoms First Approach

Solutions

Chemistry: An Atoms First Approach