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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 0.250mol of metal X at the cathode. The oxidation state of X in the molten salt is; (Given: $1 F = 96500 C {mol}^{- 1})$

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answer is C.

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Detailed Solution

Amount of electrons passed $= \frac{I t}{F} = \frac{(10.0 A) (2 \times 60 \times 60 s)}{(96500 {Cmol}^{- 1})} = 0.746 mol$

Since only 0.250mol of metal is decomposed at the cathode, the charge carried by the ion X is $z = \frac{0.746 mol}{0.250 mol} ≃ 3$

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