If the temperature is increased,which of the following reactions will proceed in the forward direction?

Dihydrogen gas is obtained from natural gas by partial oxidation with steam as per the following endothermic reaction:
$CH_{4(g)} + H_2O_{(g)} \rightleftharpoons CO_{(g)} + 3H_{2(g)}$
$(a)$ Write an expression for $K_p$ for the above reaction.
$(b)$ How will the values of $K_p$ and the composition of the equilibrium mixture be affected by:
$(i)$ increasing the pressure
$(ii)$ increasing the temperature
$(iii)$ using a catalyst?

For the equilibrium process $H_2O_{(l)} \rightleftharpoons H_2O_{(g)}$,what happens if the pressure is increased?

In the reaction $N_{2(g)} + 3H_{2(g)} \rightleftharpoons 2NH_{3(g)}$,the yield of the product increases on:

For the reaction $Cl_{2(g)} + 3F_{2(g)} \rightleftharpoons 2ClF_{3(g)}; \Delta H = -329 \, kJ$,which of the following will increase the amount of $ClF_{3(g)}$ in the equilibrium mixture?

When $I_2$ dissociates to its atomic form the following reaction occurs:
$I_{2(g)} \rightleftharpoons 2I_{(g)} ; \Delta_r H^o = +150 \ kJ \ mol^{-1}$
The forward reaction is favoured at: