Given

$2H_2{O}_{(b)}+2e^{-}{H}_{2(g)}+2O{H}_{(aq)}^{-}({10}^{-7}\frac{\text{m}\text{o}\text{l}}{L}),E=-0\mathrm{.}41V$

$C{u}_{(aq)}^{2+}+2e^{-}C{u}_{(s)},E=+0\mathrm{.}34V$

$2H_2{O}_{(b)}{O}_{2(g)}+4H_{(aq)}^{+}({10}^{-7}\frac{\text{m}\text{o}\text{l}}{L})+4e^{-},E=-0\mathrm{.}82V$

$2S{O}_{4(aq)}^{2-}{S}_2{O}_{8(aq)}^{2-}+2e^{-},E=-2\mathrm{.}01V$

$C{u}_{(s)}C{u}_{(aq)}^{2+}+2e^{-},E=-0\mathrm{.}34V$

Which of the following is produced at the cathode during the electrolysis of copper $($II$)$ sulfate solution using

copper electrodes:

a$.$ hydrogen gas

d$.$ copper atoms

b$.$ oxygen gas

e$.$ copper ions

c$.S_2{O}_8^{2-}$ ions

When platinum electrodes are used in the electrolysis of potassium iodide solution, $K{I}_{(oq)},$ the relevant half$-$

cell reactions are given below

I. $2H_2{O}_{(l)}+2e^{-}{H}_{2(g)}+2O{H}_{(aq)}^{-}({10}^{-7}\frac{\text{m}\text{o}\text{l}}{L})$

$E=-0\mathrm{.}41V$

II$.K_{(aq)}^{+}+e^{-}{K}_{(s)}$

$E=-2\mathrm{.}92V$

III. $2H_2{O}_{(l)}{O}_{2(g)}+4H_{(ag)}^{+}({10}^{-7}\frac{\text{m}\text{o}\text{l}}{L})+4e^{-}$

$E=-0\mathrm{.}815V$

IV$.2F_{(ag)}^{-}{I}_{2(s)}+2e^{-}$

$E=-0\mathrm{.}54V$

Which of these half$-$cell reactions are possible cathode reactions?

a$.$ I and IV

d$.$ I and II

b$.$ II and IV

e$.$ I and III

c$.$ III and IV

When platinum electrodes are used in the electrolysis of potassium iodide solution, $K{I}_{(29)},$ the relevant half$-$

cell reactions are given below

I. $2H_2{O}_{(l)}+2e^{-}{H}_{2(g)}+2O{H}_{(aq)}^{-}({10}^{-7}\frac{\text{m}\text{o}\text{l}}{L})$

$E=-0\mathrm{.}41V$

II$.K_{(a)}^{+}+e^{-}{K}_{(s)}$

$E=-2\mathrm{.}92V$

III. $2H_2{O}_{(l)}{O}_{2(g)}+4H_{(ag)}^{+}({10}^{-7}\frac{\text{m}\text{o}\text{l}}{L})+4e^{-}$

$E=-0\mathrm{.}815V$

IV$.2F_{(aq)}^{-}{I}_{2(s)}+2e^{-}$

$E=-0\mathrm{.}54V$

Which of these half$-$cell reactions are possible anode reactions?

a$.$ I and IV

d$.$ II and IV

b$.$ I and III

e$.$ III and IV

c$.$ I and II