.2 faraday charge is passed in 1 litre solution containing 0.1 molar Fe+3 ions. How many moles of iron get deposited at cathode assuming only iron is reduced in electrolytic process.
(E0Fe+3/Fe+2=0.77
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0.05 moles.
Explanation:
Given: .2 faraday charge is passed in 1 litre solution containing 0.1 molar Fe+3 ions.
E0Fe+3/Fe+2 = 0.77 V
E0Fe+2/Fe = -0.44V
Find: How many moles of iron get deposited at cathode assuming only iron is reduced in electrolytic process.
Solution:
E0Fe+3/Fe = -0.037V as the reduction potential of Fe3+/Fe+2 is higher initially. All FE+3 converts into Fe+2, which further gets reduced to metallic iron.
Answer is 0.05 moles.
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