Published by:
CGP EDU Academic Team
Published on: August 13, 2026
A fuel cell uses CH 4 (g) and forms CO 3 2– at the anode. It is used to power a car with 80 Amp. for 0.96 hr. How many litres of CH 4 (g) (STP) would be required ? (V m = 22.4 L/mol) (F = 96500). Assume 100% efficiency.
Text Solution
Verified by ExpertsThe correct answer is:
8
(8)
Sol. CH 4 + 10OH¯ 
CO 3 2– + 7H 2 O + 8e –
No. of Faradays required = 
Hence mol. of CH 4 required = 
x 
= 
x 
x 22.4 L = 8.356 x 0.96 = 8.02 L Ans. 8
Prepare Smarter with CGP Edu
Get practice questions, solutions, and test series in one place.
Write a Review
Share your experience with this question and solution.
Commentary
Send your comment, doubt, correction, or feedback to admin.
Similar Questions
Explore conceptually related problems
Corrosion is basically a
Rusting of iron is catalysed by which of the following
Which of the following is a highly corrosive salt
Corrosion of iron is essentially an electrochemical phenomenon where the cell reactions are
Find Eº of cell formed for rusting of iron ?
= +0.44 V
= –1.23 V
Which of the following metals could be used successfully to galvanize iron?
[Given: