Consider the following reaction for which the change in enthalpy is positive:
$2 A_{(g)} + B_{(g)} \rightleftharpoons C_{(g)} + D_{(g)}$
Which of the following will not affect the equilibrium?

Sodium sulphate dissolves in water with the evolution of heat. Consider a saturated solution of sodium sulphate. If the temperature is raised,then according to Le Chatelier's principle:

Which of the following changes will shift the reaction towards the product?
$I_{2(g)} \rightleftharpoons 2I_{(g)}$ $\Delta H_r^o(298 \ K) = +150 \ kJ$

For the reaction $CO_{(g)} + H_2O_{(g)} \rightleftharpoons CO_{2(g)} + H_{2(g)}$ at a given temperature,the equilibrium amount of $CO_{2(g)}$ can be increased by

The gaseous reaction $A(g) + B(g) \rightleftharpoons 2C(g) + D(g) + Q$ is most favoured at

Which of the following reactions will be affected by increasing the pressure? Also,mention whether the change will cause the reaction to proceed in the forward or backward direction.
$(i)$ $COCl_{2(g)} \longleftrightarrow CO_{(g)} + Cl_{2(g)}$
$(ii)$ $CH_{4(g)} + 2S_{2(g)} \longleftrightarrow CS_{2(g)} + 2H_2S_{(g)}$
$(iii)$ $CO_{2(g)} + C_{(s)} \longleftrightarrow 2CO_{(g)}$
$(iv)$ $2H_{2(g)} + CO_{(g)} \longleftrightarrow CH_3OH_{(g)}$
$(v)$ $CaCO_{3(s)} \longleftrightarrow CaO_{(s)} + CO_{2(g)}$
$(vi)$ $4NH_{3(g)} + 5O_{2(g)} \longleftrightarrow 4NO_{(g)} + 6H_2O_{(g)}$