Answer:
The volume of hydrogen gas produced is 0.104 L or 104 mL
Explanation:
In the electrolysis of dilute sulphuric acid, hydrogen gas is produced at the cathode while oxygen gas is given off at the anode in a ratio of 2:1.
At the cathode, the half reaction occurring is given as: 4H⁺(aq) + 4e⁻ ---> 2H₂(g)
From the equation of reaction, four moles of electrons are required to produce 2 moles of hydrogen gas at the cathode. Therefore, 2 moles of electrons will produce 1 mole of hydrogen gas.
1 mole of electron = 1 F = 96500 C
2 moles of electron = 193000 C
During the electrolysis experiment above, quantity of charged used, q = current(A) * time (s)
Q = 1 * 15 * 60 = 900 C
193000 C (2 moles of electron)of electricity produces 1 mole of hydrogen gas
900 C of electricity will produce 900 * 1 mole /193000 of hydrogen = 0.00466 moles of hydrogen
Molar volume of a gas at STP = 22.4 L
0.00466 moles of hydrogen occupies a volume of 0.00466 * 22.4 L = 0.104 L or 104 mL
Therefore, volume of hydrogen gas produced is 0.104 L or 104 mL
