(i) MnO₄ is the strongest oxidising agent. Oxidising power of metals decreases with a increase in their E° values.
(ii) (a) Molar conductivity of a solution is the conductance of that volume of solution containing one mole of electrolyte, kept between two electrodes having unit length joining them and large cross sectional areas so as to contain the electrolyte.
(b) The nature the electrolyte on the basis of plot is strong electrolyte. For strong electrolyte, ${\mathrm{\Lambda }}_{\mathrm{m}}^{\circ }$increases slowly with dilution.
(iii) (c) Using Debye-Huckel Onsager equation,
$\mathrm{\Lambda m}={\mathrm{\Lambda }}_{\mathrm{m}}^{\circ }-\mathrm{A}\sqrt{\mathrm{C}}$
(d) 𝚲° value from graph is 150 S cm²mol^1- .

OR

(i) Kohlrausch law:
It states that limiting molar conductivity of an electrolyte is the sum of the individual contributions of the cation and the anion of the electrolyte.
Kohlrausch observed ${\mathrm{\Lambda }}_m^0$ values for a number of strong electrolytes and found certain regularities.
Kohlrausch law of independent migration of ions is used for determination of limiting molar conductivity for weak electrolyte.
(ii) ${\mathbf{E}}_{\text{cell }}^0={\mathbf{E}}_{\text{cathode }}^0-{\mathbf{E}}_{\text{andoe }}^0$
= 0. 34 –(1.66)= 2.00 V
According to Nernst equation
$\begin{array}{l}{\mathrm{E}}_{\text{cell }}^{\circ }={\mathrm{E}}_{\text{लll }}^{\circ }-\frac{0.059}{\mathrm{n}}\log \frac{{\left[{\mathrm{Al}}^{3+}\right]}^2}{{\left[{\mathrm{Cu}}^{2+}\right]}^3}\\ {\mathrm{E}}_{\text{cell }}^0=2-\frac{0.059}{6}\log \frac{[0.15{]}^2}{[0.025{]}^2}\\ {\mathrm{E}}_{\text{cell }}^0=2-\frac{0.059}{6}(2\log 0.15-3\log 0.025)\\ {\mathrm{E}}_{\text{cell }}^0=2-\frac{0.059}{6}(-1.6478+4.8062)\\ =2-0.0311=1.9689\mathrm{V}\end{array}$