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(B) The electrolysis of acidified water involves the decomposition of water molecules into hydrogen and oxygen gases.At the cathode (negative electrod

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$2$ vol. hydrogen (cathode) and $1$ vol. oxygen (anode)

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(B) The electrolysis of acidified water involves the decomposition of water molecules into hydrogen and oxygen gases.At the cathode (negative electrode),reduction occurs: $2H^+ + 2e^- \rightarrow H_2(g)$.At the anode (positive electrode),oxidation occurs: $2H_2O(l) \rightarrow O_2(g) + 4H^+ + 4e^-$.According to the stoichiometry of the reaction $2H_2O \rightarrow 2H_2 + O_2$,for every $2$ moles of hydrogen gas produced at the cathode,$1$ mole of oxygen gas is produced at the anode.Therefore,the volume ratio of hydrogen to oxygen is $2:1$.

When a current is passed through water,acidified with a dilute sulphuric acid,the gases formed at the platinum electrodes are

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