When dilute H2SO4 is electrolyzed, hydrogen gas (H2) and oxygen gas (O2) are produced at the cathode and anode respectively. The balanced chemical equation for the electrolysis of dilute H2SO4 is:

2H2O(l) → 2H2(g) + O2(g)

This equation tells us that for every 2 moles of H2O that are electrolyzed, 2 moles of H2 and 1 mole of O2 are produced. Since the volume of a gas is directly proportional to the number of moles of the gas, we can use the ideal gas law to determine the volume of gas produced.


Given: 2F of electricity is used to electrolyze dilute H2SO4 at STP.

We know that 1 F of electricity produces 1 mole of electrons. Therefore, 2F of electricity will produce 2 moles of electrons.

Using Faraday's law of electrolysis, we can calculate the amount of H2 and O2 produced:

n(H2) = Q/F = 2F/2F = 1 mole
n(O2) = Q/2F = 2F/2F = 1 mole

Therefore, for every 2 moles of water electrolyzed, 1 mole of oxygen and 1 mole of hydrogen are produced.

Using the ideal gas law at STP (standard temperature and pressure), we can calculate the volume of gas produced:

V = nRT/P, where R is the ideal gas constant, T is the temperature in Kelvin (273 K), and P is the pressure (1 atm).

V(H2) = n(H2)RT/P = (1 mol)(0.0821 L atm/mol K)(273 K)/(1 atm) = 22.4 L
V(O2) = n(O2)RT/P = (1 mol)(0.0821 L atm/mol K)(273 K)/(1 atm) = 22.4 L

Therefore, the total volume of gas produced is:

V(total) = V(H2) + V(O2) = 22.4 L + 22.4 L = 44.8 L

Therefore, the answer is (D) 44.8 L.

It's C