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4.5g of Aluminium (at mass 27amu) is deposited at cathode from ${Al}^{3 +}$ solution by a certain quantity of electric charge. The volume of hydrogen produced at STP from $H^{+}$ ions in solution by the same quantity of electric charge will be.

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$5.6 L$

$11.2 L$

$22.4 L$

$44.8 L$

answer is C.

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Detailed Solution

Eq. of $Al = eq. of H_{2}$

$\begin{array}{l} \frac{4 .5}{\frac{27}{3}} = eq. of H_{2}; \frac{4 .5}{9} = eq. of H_{2} \\ 2 H^{+} + 2 e^{-} \to H_{2} \end{array}$

eq. of $H_{2} =$ Number of moles $x n$ factor

0.5 $= n_{H_{2}} \times 2$

$V_{H_{2}} = \frac{0 .5}{2} \times 22 .4; V_{H_{2}} = 5 .6$

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