JEE Main 2014 · 9 Apr · Shift 1 · Chemistry Q37

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ChemistrySingle correct+4 / -1Question 37 of 90

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)

Answer and worked solution

Official answer: C

$Q=10\times7200=72000$ C, i.e. $\frac{72000}{96500}=0.746$ mol of electrons. Per mole of metal: $\frac{0.746}{0.250}\approx3$ , so the oxidation state is +3.

Topics:Electrolysis and Faraday's laws

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JEE Main 2014 · 9 Apr · Shift 1, Chemistry question 37