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(D) According to Faraday's law of electrolysis,the number of gram equivalents of $Al$ deposited is equal to the number of gram equivalents of $H_2$ pr

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$5.6$

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(D) According to Faraday's law of electrolysis,the number of gram equivalents of $Al$ deposited is equal to the number of gram equivalents of $H_2$ produced.Gram equivalents of $Al = \frac{	ext{mass}}{	ext{equivalent mass}} = \frac{4.5}{27/3} = \frac{4.5}{9} = 0.5 \ eq$.Since the amount of electricity is the same,gram equivalents of $H_2 = 0.5 \ eq$.Number of moles of $H_2 = \frac{	ext{gram equivalents}}{	ext{n-factor}} = \frac{0.5}{2} = 0.25 \ mol$.Volume of $H_2$ at $STP = 	ext{moles} 	imes 22.4 \ L/mol = 0.25 	imes 22.4 = 5.6 \ L$.

When a certain amount of electricity is passed through a solution of $Al^{3+}$,$4.5 \ g$ of aluminum (atomic mass $27 \ amu$) is deposited at the cathode. If the same amount of electricity is passed through $H^{+}$ ions,what volume of hydrogen (in $L$) is produced at $STP$?

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