4.5 g of aluminium (at. mass 27 amu) is deposited at cathode from a molten electrolyte containing Al3+ ions by a certain quantity of electric charge. The volume of hydrogen produced at STP from H+ ions in a solution by the same quantity of electric charge will be

Question

4.5 g of aluminium (at. mass 27 amu) is deposited at cathode from a molten electrolyte containing Al3+ ions by a certain quantity of electric charge. The volume of hydrogen produced at STP from H+ ions in a solution by the same quantity of electric charge will be (A) 44.8 L (B) 11.2 L (C) 22.4 L (D) 5.6 L

Tardigrade Admin · Accepted Answer

From second law of Faraday (m Al /m H ) =(E Al /E H ) (4.5/m H ) =(27 / 3/1) or m H =0.5 g ∵ Volume of 2 g H 2 at STP =22.4 L ∴ Volume of 0.5 g H 2 at STP =(22.4 × 0.5/2) L =5.6 L

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

44.8 L

11.2 L

22.4 L

5.6 L

From second law of Faraday
$\frac{m _{A l}}{m _{H}} = \frac{E _{A l}}{E _{H}}$
$\frac{4.5}{m _{H}} = \frac{27/3}{1}$
or $m_{H} = 0.5 g$
$∵$ Volume of $2 g H_{2}$ at STP $= 22.4 L$
$∴$ Volume of $0.5 g H_{2}$ at STP
$= \frac{22.4 \times 0.5}{2} L = 5.6 L$

Q. 4.5g of aluminium (at. mass 27 amu) is deposited at cathode from a molten electrolyte containing Al3+ ions by a certain quantity of electric charge. The volume of hydrogen produced at STP from H+ ions in a solution by the same quantity of electric charge will be