Question

A current of $2amp$ when passed for $5$ hour through a molten salt deposits $22.2g$ of metal of atomic mass $177$. Then calculate the positive oxidation state of the metal in the metal salt.

Answer 1

$I=2A$

$t=5hr=5\times 3600=18000s$

moles deposited $=0.1254$

charge passed $=It=36000C$

Let $1$ mole has $n$ moles of $Hu$ charge.

Then, $n\times (0.1254\times 6.022\times {10}^{23})\times (1.6\times {10}^{-19}C)=3600C⟹n=\frac{3600}{1.6\times 6.022\times 0.1254\times {10}^4}=0.297$

$\therefore$ The oxidation state $=0.297$