For an exothermic reaction,the equilibrium constant:

The role of a catalyst in a reversible reaction is to

Which of the following changes will not alter the equilibrium concentration of ammonia in the reaction: $N_{2(g)} + 3H_{2(g)} \rightleftharpoons 2NH_{3(g)} \quad \Delta H = -x \text{ kJ}$?

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?

For the following reaction,which change will shift the equilibrium towards the product?
$I_{2(g)} \rightleftharpoons 2I_{(g)}; \Delta H_r^o(298 \ K) = +150 \ kJ$

In the equilibrium $N_2 + 3H_2 \rightleftharpoons 2NH_3 + 22 \ kcal$,the formation of ammonia is favoured by