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An aqueous solution of NaCl is electroly...

An aqueous solution of `NaCl` is electrolysed with inert electrodes. Write the equations for the reactions taking place at cathode and anode. What happens if `AgNO_(3(aq.))` is used instead of `NaCl`?

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To solve the question, we will break it down into two parts: the electrolysis of an aqueous solution of NaCl and the electrolysis of an aqueous solution of AgNO3. ### Part 1: Electrolysis of Aqueous NaCl 1. **Identify the electrodes**: In this case, we are using inert electrodes, which do not participate in the reaction but allow the passage of current. 2. **Anode Reaction**: At the anode, oxidation occurs. In the case of NaCl, water is oxidized to produce oxygen gas. The half-reaction can be written as: \[ ...
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Knowledge Check

  • Brine is electrolysed by using inert electrodes. The reaction at anode is

    A
    `Cl^(-)(aq) to 1//2 Cl_2(g) + e^(-) , E_("cell")= 1.36V`
    B
    `2H_2O (l) to O_2(g) + 4H^(+) (aq)^(+) 4e^(-) , E_("cell") = 1.23 V`
    C
    `Na^(+) (aq) + e^(-) to Na(s) , E_("cell") = 2.71V`
    D
    `H^(+)(aq) + e^(-) to 1//2 H_2(g) , E_("cell") = 0.00V`

  • Brine is electrolysed by using inert electrodes. The reaction at anode is

    A
    `Cl^(-)(aq) to 1//2 Cl_2(g) + e^(-) , E_("cell")= 1.36V`
    B
    `2H_2O (l) to O_2(g) + 4H^(+) (aq)^(+) 4e^(-) , E_("cell") = 1.23 V`
    C
    `Na^(+) (aq) + e^(-) to Na(s) , E_("cell") = 2.71V`
    D
    `H^(+)(aq) + e^(-) to 1//2 H_2(g) , E_("cell") = 0.00V`

  • Brine is electrolysed by using inert electrodes. The reaction at anode is

    A
    `Cl^(-)(aq) to 1//2 Cl_2(g) + e^(-) , E_("cell")= 1.36V`
    B
    `2H_2O (l) to O_2(g) + 4H^(+) (aq)^(+) 4e^(-) , E_("cell") = 1.23 V`
    C
    `Na^(+) (aq) + e^(-) to Na(s) , E_("cell") = 2.71V`
    D
    `H^(+)(aq) + e^(-) to 1//2 H_2(g) , E_("cell") = 0.00V`

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