A current of 2.0 A passed for 5 hours through a molten metal salt deposits 22.2 g of metal (At. wt. = 177). The oxidation state of the metal in the metal salt is:

Q. A current of 2.0 A is passed for 5 hours through a molten metal salt deposits 22.2 g of metal (At. mass: 177 u). The oxidation states of the metal in metal salt is:

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A current of 2 amp when passed for 5 hours through a molten salt deposits 22.2 g of metal of atomic mass 177. The oxidation state of the metal in the metal salt is:

The correct option is C +3W=ItE96500E=W×96500It=22.2×965002×5×3600=59.5Equivalent mass =Atomic massOxidation state59.5=177n∴n≈3.

A current of $2 a m p$ when passed for $5$ hours through a molten salt deposits $22.2 g$ of metal of atomic mass $177$ . The oxidation state of the metal in the metal salt is:

The correct option is C $+ 3$
$W = \frac{I t E}{96500}$
$E = \frac{W \times 96500}{I t} = \frac{22.2 \times 96500}{2 \times 5 \times 3600} = 59.5$
Equivalent mass $= \frac{A t o m i c m a s s}{O x i d a t i o n s t a t e}$
$59.5 = \frac{177}{n}$
$∴ n \approx 3$ .