Determine the time needed to liberate 1.0 litre of hydrogen at STP in an electrolytic cell using a current of 5.0 A .

Step-by-step solution

The reaction for the liberation of hydrogen gas at the cathode is: 2H⁺ + 2e⁻ H₂ From the stoichiometry, 2 moles of electrons ( 2 F of charge) are required to produce 1 mole of H₂ gas. At STP, 1 mole of an ideal gas occupies 22.4 L . Number of moles of H₂ in 1.0 L is 1.0 22.4 mol . Charge required, Q = 2 1.0 22.4 96500 C = 96500 11.2 C . Using the formula Q = I t , where I = 5.0 A : t = Q I = 96500 11.2 5.0 s = 19300 11.2 s 1723.2 s Converting time into minutes: t = 1723.2 60 minutes 28.72 minutes This is approximat