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Calculate the volume of H2 and O2 evolved at the electrode when Nacl is electrolysed using graphite electrodes at STP when 0.5 F electricity was released.

Chemistry

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  1. Write the half-reactions for the electrolysis of NaOH\text{NaOH} solution using graphite electrodes.

    At the cathode (reduction): Water is reduced to hydrogen gas and hydroxide ions.

    2H2O(l)+2e−→H2(g)+2OH−(aq)2\text{H}_2\text{O}(l) + 2e^- \to \text{H}_2(g) + 2\text{OH}^-(aq)

    At the anode (oxidation): Hydroxide ions are oxidized to oxygen gas and water.

    4OH−(aq)→O2(g)+2H2O(l)+4e−4\text{OH}^-(aq) \to \text{O}_2(g) + 2\text{H}_2\text{O}(l) + 4e^-

  2. Determine the moles of electrons passed.

    The quantity of electricity released is 0.5 F0.5 \, \text{F}.
    One Faraday (1 F1 \, \text{F}) corresponds to 1 mole of electrons.
    Therefore, moles of electrons passed =0.5 mol e−= 0.5 \, \text{mol } e^-.

  3. Calculate the moles of H2\text{H}_2 produced.

    From the cathode reaction, 2 moles of electrons produce 1 mole of H2\text{H}_2.

    Moles of H2=0.5 mol e−×1 mol H22 mol e−=0.25 mol H2\text{Moles of H}_2 = 0.5 \, \text{mol } e^- \times \frac{1 \, \text{mol H}_2}{2 \, \text{mol } e^-} = 0.25 \, \text{mol H}_2

  4. Calculate the moles of O2\text{O}_2 produced.

    From the anode reaction, 4 moles of electrons produce 1 mole of O2\text{O}_2.

    Moles of O2=0.5 mol e−×1 mol O24 mol e−=0.125 mol O2\text{Moles of O}_2 = 0.5 \, \text{mol } e^- \times \frac{1 \, \text{mol O}_2}{4 \, \text{mol } e^-} = 0.125 \, \text{mol O}_2

  5. Convert moles of gases to volume at STP.

    At STP (Standard Temperature and Pressure), 1 mole of any ideal gas occupies 22.4 L22.4 \, \text{L}.

    Volume of H2\text{H}_2:

    Volume of H2=0.25 mol×22.4 L/mol=5.6 L\text{Volume of H}_2 = 0.25 \, \text{mol} \times 22.4 \, \text{L/mol} = 5.6 \, \text{L}

    Volume of O2\text{O}_2:

    Volume of O2=0.125 mol×22.4 L/mol=2.8 L\text{Volume of O}_2 = 0.125 \, \text{mol} \times 22.4 \, \text{L/mol} = 2.8 \, \text{L}

    The volume of H2\text{H}_2 released is 5.6 L\boxed{\text{5.6 L}} and the volume of O2\text{O}_2 released is 2.8 L\boxed{\text{2.8 L}}.

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