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An equeous solutioon of NaCI is electrol...

An equeous solutioon of `NaCI` is electrolysed with inert electrodes. Write the equations for the reactions taking place at cathode and anode. What happens if `aNO_(3(eq.))` is used instead of `NaCI`?

Text Solution

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For `NaCI_((eq)), anode: 2CI^(-) rarr CI_(2) +2e^(-)`
`{:(,"cathode",:,2H^(+)+2e^(-),rarrH_(2)),("For"NaNO_(3(eq)),"anode",:,2OH^(-)rarr,H_(2)O+(1)/(2)O_(2)+2e^(-)),(,"cathode",:,2H^(+)+2e^(-),rarrH_(2)):}`
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Knowledge Check

  • If aqueous solutions of AgNO_3 is electrolysed using inert electrode the gas evolved at anode is .

    A
    ` NO_2`
    B
    `O_2`
    C
    ` H_2`
    D
    `N_2O`

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

    A
    `Cl^(-)(aq.)rarr(1)/(2)Cl_(2)(g)+e^(-), E_("cell")^(o.)=1.36 V`
    B
    `2H_(2)O(l)rarr O_(2)(g)4H^(+)+4e^(-), E_("cell")^(o.)=1.23V`
    C
    `Na^(+)(aq.)+e^(-)rarr Na(s), E_("cell")^(o.)=2.71 V`
    D
    `H^(+)(aq.)+e^(-)rarr(1)/(2)H_(2)(g),E_("cell")^(o.)=0.00V`

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

    A
    `Cl^(-) (a) to (1)/(2) Cl_(2)(g) +e^(-), " "E_("cell")^(0) = 1.36V`
    B
    `2H_(2)O(l) to O_(2)(g)+4H^(+)+4e^(-), " "E_("cell")^(0) = 1.23V`
    C
    `Na^(+) (aq) +e^(-) to Na (s), " "E_("cell")^(0) = 2.71V`
    D
    `H^(+)(aq) + e^(-) to (1)/(2)H_(2) (g), " "E_("cell")^(0) = 0.00V`

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