Chemistry · 2014
JEE Main · 9 April 2014, Shift 1 · Q37
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…
A current of $\displaystyle 10.0$ A flows for $\displaystyle 2.00$ h through an electrolytic cell containing a molten salt of metal X. This results in the decomposition of $\displaystyle 0.250$ mol of metal X at the cathode. The oxidation state of X in the molten salt is : $\displaystyle (\mathrm{F}=96,500 \mathrm{C})$
Official answer
(3)
$\displaystyle 3$ +
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JEE Main 2014 Chemistry question, with the answer from NTA’s final answer key. Where our answers come from.