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  4. A current of 10.0 A flows for 2.00 h through an electrolytic cell containing a molten salt of metal X. This results in the decomposition of 0.250 mol of metal X at the cathode. The oxidation state of X in the molten salt is: (F = 96,500 C)

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Q. A current of $10.0 \,A$ flows for $2.00 \,h$ through an electrolytic cell containing a molten salt of metal $X$. This results in the decomposition of $0.250 \,mol$ of metal $X$ at the cathode. The oxidation state of $X$ in the molten salt is : $(F = 96,500 \,C)$

JEE MainJEE Main 2014Electrochemistry

Solution:

$w=\frac{E}{96500}\times It$

$\Rightarrow $ No. of moles $=\frac{It}{96500\times\left(n-factor\right)}$

$\Rightarrow 0.25=\frac{10\times2\times60\times60}{96500\times \text{n-factor}}$

$\Rightarrow $ n - factor $=\frac{720\times4}{965} =3$

$\therefore $ Oxidation state of molten salt is $+3$