`4.5 g` of aluminium (at mass `27 u`) is deposited at cathode from `Al^(3+)` solution by a certain quantity of electric charge. The volume of hydrogen gas produced at `STP` from `H^(+)` ions in solution by the same quantity of electric charge will be:

Options

A. `44.8` L
B. `22.4 L`
C. `11.2 L`
D. 5.6 L

Answer

D

Explanation

Gram equivalent of `H^(+)` = Gram equivalent of `Al^(3+)`
No. of gm equivalents of `Al^(3+) = (4.5)/(9) = 0.5`
No. of gm equivalents of `H^(+)` = No. of mol of `H^(+)`
`therefore` Mass of `H^+ = 0.5 xx 1 = 0.5` g
Now 2 g of `H_(2)` at STP = 22.4 L
0.5 g of `H_(2)` at STP = `(22.4 xx 0.5)/(2)`
=`5.6`L