For the reaction $N_{2(g)} + 3H_{2(g)} \rightleftharpoons 2NH_{3(g)} + 21.9 \ kcal$,which conditions favor the production of ammonia?

Consider the reaction equilibrium,$2SO_{2(g)} + O_{2(g)} \rightleftharpoons 2SO_{3(g)}$; $\Delta H^\circ = -198 \ kJ$. On the basis of Le Chatelier's principle,the condition favourable for the forward reaction is

In which of the following equilibrium systems is the rate of the backward reaction favoured by an increase of pressure?

In the equilibrium $N_{2(g)} + 3H_{2(g)} \rightleftharpoons 2NH_{3(g)} + 22 \ kcal$,the formation of ammonia is favored by:

The reaction,$N_{2(g)} + 3H_{2(g)} \rightleftharpoons 2NH_{3(g)}$ is exothermic and reversible. $A$ mixture of $N_{2(g)}$,$H_{2(g)}$,and $NH_{3(g)}$ is at equilibrium in a closed container. When a certain quantity of extra $H_{2(g)}$ is introduced into the container,while keeping the volume constant,then which statement among the following is true?

In which of the following reactions will the amount of products not increase upon increasing the pressure?