Chapter 21, Problem 81PS

### Chemistry & Chemical Reactivity

10th Edition
John C. Kotz + 3 others
ISBN: 9781337399074

Chapter
Section

### Chemistry & Chemical Reactivity

10th Edition
John C. Kotz + 3 others
ISBN: 9781337399074
Textbook Problem

# If an electrolytic cell for producing F2 (Figure 21.34) operates at 5.00 × 103 A (at 10.0 V), what mass of F2 can be produced per 24-hour day? Assume the conversion of F− to F2 is 100%.

Interpretation Introduction

Interpretation:

To calculate the mass of F2 produced per-24 hour a day in an electrolytic cell.

Concept introduction:

The Fraday’s first law of electrolysis state that the mass of the substance (m) deposited at any electrode is directly proportional to the charge (Q) passed. The mathematical form of the Fraday’s first law is written as’

m=(QF)(MZ)

Here,

The symbol F is the Faraday’s constant.

The symbol M is the molar mass of the substance in grams per mol.

The symbol Z is the valancy number of ions of the substance (electrons transferred per ion).

In the simple case of constant current electrolysis, Q=I×t leading to

m=(I×tF)(MZ) (1)

Here, t is the total time the constant current (I) is applied.

Explanation

The mass of F2 produced per-24 hour a day in an electrolytic cell is calculated below.

Given:

The constant current I=5Ã—103â€‰A.

The time t is 86400â€‰s.

The molar mass of F2 is 37.99â€‰gâ‹…molâˆ’1.

The faradayâ€™s constant F is equal to 96500â€‰Câ‹…molâˆ’1.

The reaction of flouride ion to produce flourine is written as,

Â Â Â Â 2Fâˆ’(aq)â†’F2(g)+2eâˆ’

Here, Z=2

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