Molar conductivity ($$\Lambda $$_m) of aqueous solution of sodium stearate, which behaves as a strong electrolyte, is recorded at varying concentrations (C) of sodium stearate. Which one of the following plots provides the correct representation of micelle formation in the solution?

(critical micelle concentration (CMC) is marked with an arrow in the figures)

For the following cell,

$$Zn\left( s \right)\left| {ZnS{O_4}\left( {aq} \right)} \right|\left| {CuS{O_4}\left( {aq} \right)} \right|Cu\left( s \right)$$

when the concentration of $$Z{n^{2 + }}$$ is $$10$$ times the concentration of $$C{u^{2 + }},$$ the expression for $$\Delta G$$ (in $$J\,mo{l^{ - 1}}$$) is [$$F$$ is Faraday constant; $$R$$ is gas constant; $$T$$ is temperature; $${E^0}$$ (cell)$$=1.1$$ $$V$$]

For the following electrochemical cell at 298 K
Pt(s) | H₂ (g, 1 bar) | H⁺ (aq, 1 M) || M⁴⁺ (aq), M²⁺ (aq) | Pt (s)
E_cell = 0.092 V when $${{\left[ {{M^{2 + }}(aq)} \right]} \over {\left[ {{M^{4 + }}(aq)} \right]}}$$ = 10^x
Give, $$E_{{M^{4 - }}/{M^{2 + }}}^o$$ = 0.151 V; 2.303 RT/F = 0.059 V

The value of x is

The standard reduction potential data at 25^oC is given below:
E^o (Fe³⁺ , Fe²⁺) = +0.77V;
E^o (Fe²⁺ , Fe) = -0.44V;
E^o (Cu²⁺ , Cu) = +0.34V;
E^o (Cu⁺ , Cu) = +0.52V;
E^o [O₂(g) + 4H⁺ + 4e^- $$\to$$ 2H₂O] = +1.23V;
E^o [O₂(g) + 2H₂O + 4e^- $$\to$$ 4OH^-] = +0.40 V
E^o (Cr³⁺ , Cr) = -0.74V;
E^o (Cr²⁺ , Cr) = -0.91V;

Match E^o of the redox pair in List – I with the values given in List – II and select the correct answer using the code given below the lists:

List - I
P. E^o (Fe³⁺ , Fe)
Q. E^o (4H₂O $$\leftrightharpoons$$ 4H⁺ + 4OH^-)
R. E^o (Cu²⁺ + Cu $$\to$$ 2Cu⁺)
S. E^o (Cr³⁺, Cr²⁺)

List - II
1. -0.18 V
2. -0.4 V
3. -0.04 V
4. -0.83 V