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Question

How many hours does it take to reduce $$3$$ moles of $${Fe}^{3+}$$ to $${Fe}^{2+}$$ with $$2.0A$$ current intensity?


Solution

Given, Current $$=2.0$$ Ampere
$$3{ Fe }^{ 3+ }+3{ e }^{ - }\longrightarrow 3{ Fe }^{ 2+ }$$
Charge required $$= Faraday =3\times 96500$$ coulomb
                            $$=289500$$ coulomb
We know, $$Charge=Current\times Time$$
or Time $$=\cfrac{289500}{2}$$
              $$=144750$$ sec
              $$=40.20$$ hrs.

Chemistry

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