The cell that will measure the standard electrode potential of a copper electrode is:

An electrochemical cell can behave like an electrolytic cell when -

1. E_cell = 0

2. E_cell > E_ext

3. E_ext > E_cell

4. E_cell = E_ext

The half-cell reaction at the anode during the electrolysis of aqueous sodium chloride solution  is represented by : 

1. Na⁺(aq) + e^- ⟶ Na(s) ; \(E_{cell}^{o} \ = \ -2.71 \ V \)

2. 2H₂O(l) ⟶ O₂(g) + 4H⁺(aq) + 4e^- ; \(E_{cell}^{o} \) = 1.23 V

3. H⁺(aq) + e^- ⟶ \(\frac{1}{2}\)H₂(g) ; \(E_{cell}^{o} \) = 0.00 V

4. Cl^-(aq) ⟶ \(\frac{1}{2}\)Cl₂(g) + e- ; \(E_{cell}^{o}\) $= 1.\mathrm{36 }\mathrm{V}$

The positive value of the standard electrode potential of Cu²⁺ / Cu indicates that-

${\mathrm{E}}_{\mathrm{Cell}}^{°}$ of some half cell reactions are given below. 

I:  \(\mathrm{H}^{+} (a q)+e^{-} \rightarrow \frac{1}{2} \mathrm{H}_2 (g )\quad ; \quad E_{\text {cell }}^0=0.00 \mathrm{~V} \)
II: \(2 \mathrm{H}_2 \mathrm{O(l)} \rightarrow O_2 (g)+4 \mathrm{H}^{+} (a q)+4 e^{-} ; E_{\text {cell }}^{0}=1.23 \mathrm{~V} \)
III: \(2 \mathrm{SO}_4^{2-} (a q) \rightarrow \mathrm{S}_2 \mathrm{O}_8^{2-} (a q)+2 e^{-}, E_{\text {cell }}^{0}=1.96 \mathrm{~V} \)

The correct statements among the following are:

1. (a, b)
2. (b, c)
3. (c, d)
4. (a, c)

What will happen during the electrolysis of aqueous solution of CuSO₄ in the presence of Cu electrodes?

The correct choice among the given is -

For the given cell, Mg | Mg²⁺ || Cu²⁺ | Cu

a.  Mg acts as cathode

b.  Cu acts as cathode

c.  The cell reaction is   \(Mg + Cu^{2+} \rightarrow Mg^{2+} + Cu\)

d.  Cu is the oxidising agent

The correct choice among the given is - 

Given below are two statements: 

Given below are two statements: