For the balanced reaction $2SO_2(g) + O_2(g) \rightleftharpoons 2SO_3(g) + \text{Heat}$,which of the following conditions will favor the forward reaction?

Formation of $SO_3$ takes place according to the reaction:
$2SO_2(g) + O_2(g) \rightleftharpoons 2SO_3(g); \,\, \Delta H = -45.2 \, kcal$
Which of the following factors favours the formation of $SO_3$?

In which of the following reactions at equilibrium,the position of the equilibrium shifts towards the products,if the total pressure is increased?
$(I)$ $X_{2(g)} + 3Y_{2(g)} \rightleftharpoons 2XY_{3(g)}$
$(II)$ $X_{2(g)} + Y_{2(g)} \rightleftharpoons 2XY_{(g)}$
$(III)$ $X_{2(g)} + Z_{2(g)} \rightleftharpoons 2XZ_{(g)}$
$(IV)$ $X_{2(g)} + Y_{4(g)} \rightleftharpoons 2XY_{2(g)}$

Raising the temperature of an equilibrium system:

For the reaction at equilibrium
$N_{2(g)} + 3H_{2(g)} \rightleftharpoons 2NH_{3(g)}$
On addition of an inert gas at constant pressure and constant temperature,which of the following changes is $NOT$ observed?

For the reaction $SO_{2(g)} + 1/2 O_{2(g)} \rightleftharpoons SO_{3(g)}$,the percentage yield of product at different pressures is shown in the figure. Then,which among the following is true?