Propane in presence of O ₂ gas undergoes complete combustion to produce CO ₂ and H ₂ O . The required O ₂ for this combustion reaction was produced by the electrolysis of water. For what duration of time had water been electrolysed by passing 200 ~A current so that Oxygen gas produced could completely burn 44 ~g of Propane?

Step-by-step solution

The balanced chemical equation for the combustion of propane is: C ₃ H ₈ + 5 O ₂ 3 CO ₂ + 4 H ₂ O The molar mass of propane ( C ₃ H ₈ ) is 3 12 + 8 1 = 44 g/mol . Moles of propane = 44 g 44 g/mol = 1 mol . From the stoichiometry, 1 mol of propane requires 5 mol of O ₂ . The electrolysis of water is given by: 2 H ₂ O 2 H ₂ + O ₂ For 1 mol of O ₂ produced, 4 moles of electrons are required (since each oxygen atom changes oxidation state from -2 to 0 , and there are 2 oxygen atoms per O ₂ molecule). Total moles of ele