In which of the following equilibrium reactions,the equilibrium would shift to the right,if total pressure is increased?

On the basis of the $Le \ Chatelier$ principle,explain how temperature and pressure can be adjusted to increase the yield of ammonia in the following reaction: $N_{2(g)} + 3H_{2(g)} \rightleftharpoons 2NH_{3(g)}$; $\Delta H = -92.38 \ kJ \ mol^{-1}$. What will be the effect of the addition of argon to the above reaction mixture at constant volume?

According to Le Chatelier's principle,an increase in the temperature of the following reaction will:
$N_2 + O_2 \rightleftharpoons 2NO - 43,200 \ kcal$

In the reaction ${A_2}_{(g)} + 4{B_2}_{(g)} \rightleftharpoons 2A{B_4}_{(g)}$ where $\Delta H < 0$,the formation of $AB_{4(g)}$ will be favoured by:

Observe the following equilibrium:
$Fe^{3+}_{(aq)} + SCN^{-}_{(aq)} \rightleftharpoons [Fe(SCN)]^{2+}_{(aq)}$
(yellow) (colorless) (deep red)
Addition of aqueous oxalic acid solution to the above equilibrium:

For the reaction $X_{2(g)} + 4Y_{2(g)} \rightleftharpoons 2XY_{4(g)}$,$\Delta H < 0$. According to which of the following factors is the yield of the product favored?