For the following gaseous reversible reaction:
$3\text{A}_{(g)} + \text{B}_{(g)} \rightleftharpoons \text{A}_3\text{B}_{(g)} \quad (\Delta_r H = -q\text{ kJ})$. The amount of product $\text{A}_3\text{B}_{(g)}$ is affected by ____

For the reversible reaction,
$\text{N}_{2(g)} + 3\text{H}_{2(g)} \rightleftharpoons 2\text{NH}_{3(g)}$
When the partial pressure is measured in atmosphere, the value of $K_p$ at $500^\circ\text{C}$ is $1.44 \times 10^{-5}$. The value of $K_c$ when the concentration is expressed in mol L$^{-1}$ is:

Which of the following statements is/are true about equilibrium?

(a) Equilibrium is possible only in a closed system of at a given temperature

(b) All the measurable properties of the system remain constant at equilibrium

(c) Equilibrium constant for the reverse reaction is the inverse of the equilibrium constant for the reaction in the forward direction.

According to Le Chatelier's principle, in the reaction $\mathrm{CO}(\mathrm{g})+3 \mathrm{H}_2(\mathrm{~g}) \rightleftharpoons \mathrm{CH}_4(\mathrm{~g})+\mathrm{H}_2 \mathrm{O}(\mathrm{g})$, the formation of methane is favoured by

(a) Increasing the concentration of CO

(b) Increasing the concentration of $\mathrm{H}_2 \mathrm{O}$

(c) Decreasing the concentration of $\mathrm{CH}_4$

(d) Decreasing the concentration of $\mathrm{H}_2$