4.5 g of aluminium (at. mass 27u) is deposited at cathode from Al3+ solution by 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

Question

4.5 g of aluminium (at. mass 27u) is deposited at cathode from Al3+ solution by 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 (A) 22.4 L (B) 44.8 L (C) 5.6 L (D) 11.2 L

Tardigrade Admin · Accepted Answer

From second law of Faraday (mAl/mH)=(EAl/EH) ∴ (4.5/mH)=(27/3/1) or mH=0.5 g ∵ The volume of 2 g H2 at STP = 22.4 L ∴ The volume of 0.5 g Hz at STP =(22.4× 0.5/2)L=5.6 L

Q. 4.5 g of aluminium (at. mass 27u) is deposited at cathode from $A l^{3 +}$ solution by 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

22.4 L

44.8 L

5.6 L

11.2 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 $m_{H} = 0.5 g$ $∵$ The volume of 2 g $H_{2}$ at STP = 22.4 L $∴$ The volume of 0.5 g Hz at STP $= \frac{22.4 \times 0.5}{2} L = 5.6 L$

Q. 4.5 g of aluminium (at. mass 27u) is deposited at cathode from Al3+ solution by 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