Which of the following plots represent an exothermic reaction?

Equilibrium constants $K_1$ and $K_2$ for the following equilibria are given:
$NO_{(g)} + 1/2 O_{2(g)} \rightleftharpoons NO_{2(g)}$
$2NO_{2(g)} \rightleftharpoons 2NO_{(g)} + O_{2(g)}$
What is the relationship between $K_1$ and $K_2$?

What is the relationship between $K_{p}$ and $K_{c}$ when $\Delta n = 0$,$\Delta n > 0$,and $\Delta n < 0$?

For the following given equilibrium reaction,$\frac{K_{c}}{K_{p}}$ is equal to $1076$ at $T \ K$. What is the value of $T$ (in $K$)? $(R = 0.082 \ L \ atm \ K^{-1} \ mol^{-1})$
$N_{2(g)} + 3H_{2(g)} \rightleftharpoons 2NH_{3(g)}$

For which of the following equilibria are $K_P$ and $K_C$ different?

For the equilibrium,$2 \ NOCl \ (g) \rightleftharpoons 2 \ NO \ (g) + Cl_{2} \ (g)$,the value of the equilibrium constant,$K_{c}$ is $3.75 \times 10^{-6}$ at $1069 \ K$. Calculate the $K_{p}$ for the reaction at this temperature?