Relation Between equilibrium constant calculated from partial pressure and molar concentration.

In a $0.25$ litre tube, dissociation of $4$ moles of $\mathrm{NO}$ takes place. If its degree of dissociation is $10\%$, the value of ${\mathrm{K}}_{\mathrm{p}}$ for reaction $\begin{array}{cccc}2\mathrm{NO} \left(\mathrm{g}\right)& \rightleftharpoons & {\mathrm{N}}_{2 }\left(\mathrm{g}\right)+& {\mathrm{O}}_2\end{array}\left(\mathrm{g}\right)$ is:

At $1000 \mathrm{K}$, the value of ${\mathrm{K}}_{\mathrm{p}}$ for the reaction:
$\mathrm{A} \left(\mathrm{g}\right)+2\mathrm{B} \left(\mathrm{g}\right)\rightleftharpoons 3\mathrm{C} \left(\mathrm{g}\right)+\mathrm{D} \left(\mathrm{g}\right)$ is $0.05$ atmosphere. The value of ${\mathrm{K}}_{\mathrm{C}}$ in terms of $\mathrm{R}$ would be:

For the reaction:

${\mathrm{CuSO}}_4·5{\mathrm{H}}_2\mathrm{O} \left(\mathrm{s}\right)\rightleftharpoons {\mathrm{CuSO}}_4·3{\mathrm{H}}_2\mathrm{O} \left(\mathrm{s}\right)+2{\mathrm{H}}_2\mathrm{O} \left(\mathrm{g}\right)$

Which one is correct representation?

For which reaction is ${\mathrm{K}}_{\mathrm{p}}={\mathrm{K}}_{\mathrm{C}}:$

For the following gases equilibrium, ${\mathrm{N}}_2{\mathrm{O}}_4( \mathrm{g})\rightleftharpoons 2{\mathrm{NO}}_2( \mathrm{g}), {\mathrm{K}}_{\mathrm{p}}$ is found to be equal to ${\mathrm{K}}_{\mathrm{c}}$. This is attained when:

$\log \frac{{\mathrm{K}}_{\mathrm{p}}}{{\mathrm{K}}_{\mathrm{c}}}+\log \mathrm{RT}=0$ is a relationship for the reaction: