A. 1.00F
B. 0.01F
C. 0.05F
D. 0.50F
Correct Answer:
Option D = 0.50F
Explanation
Cu → Cu²+ + 2e
1 mole Cu requires 2f
0.25 mole Cu requires x
x = 0.25×2/1 = 0.50f
How many faraday of electricity is required to produce 0.25 mole of copper?
![What mass of copper will be deposited by the liberation of Cu2+ when 0.1F of electricity flows through an aqueous solution of a copper (ll) salt? [Cu = 64]](https://erudites.ng/wp-content/plugins/contextual-related-posts/default.png "What mass of copper will be deposited by the liberation of Cu2+ when 0.1F of electricity flows through an aqueous solution of a copper (ll) salt? [Cu = 64]")
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