The equilibrium of the reaction $2A_{(s)} + 3B_{(g)} \rightleftharpoons 3C_{(g)} + D_{(g)} + Q$ is represented as shown. If the pressure on the system is reduced to half of its original value,then:

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

The formation of nitric oxide by the reaction $N_2 + O_2 \rightleftharpoons 2NO$ with $\Delta H = +43.200 \ kcal$ is favoured by:

What is the optimum temperature maintained in the Haber process for the production of ammonia (in $K$)?

In which of the following equilibria does a change in the volume of the system not alter the number of moles?

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