(may be broke/outdated!)
How many coulombs of electrical charge must pass through an electrolytic cell to reduce 0.82 moles of Ca2+ ion to calcium metal?
a) 3.9e3
b) 1.6e5
c) 7.9e4
d) 4.2e–6
e) 4.0e4
I got b, 96500 x 2 = 193000 x .82 = 158260 …im not sure Im doing this right…
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One Response
The answer is b however I don’t quite follow your reasoning
Faraday’s constant is approximately 96500 coulomb/mole of electrons
Each Ca2+ needs 2 electrons so 0.82 mole Ca2+ need 2*0.82 mole of elecrons, so a total charge of 2*0.82*F=2*0.82*96500= 1.6*10^5