The reaction $2SO_{2(g)} + O_{2(g)} \rightleftharpoons 2SO_{3(g)} + q$ is favored by:

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.
$(i)$ $COCl_{2(g)} \longleftrightarrow CO_{(g)} + Cl_{2(g)}$
$(ii)$ $CH_{4(g)} + 2S_{2(g)} \longleftrightarrow CS_{2(g)} + 2H_2S_{(g)}$
$(iii)$ $CO_{2(g)} + C_{(s)} \longleftrightarrow 2CO_{(g)}$
$(iv)$ $2H_{2(g)} + CO_{(g)} \longleftrightarrow CH_3OH_{(g)}$
$(v)$ $CaCO_{3(s)} \longleftrightarrow CaO_{(s)} + CO_{2(g)}$
$(vi)$ $4NH_{3(g)} + 5O_{2(g)} \longleftrightarrow 4NO_{(g)} + 6H_2O_{(g)}$

In a reversible reaction at $300 \ K$,$K_c > K_p$ and $\Delta H = +40 \ kcal$. The product will be obtained in a higher amount on:

When an orange solution containing $Cr_{2}O_{7}^{2-}$ ions is treated with an alkali,a yellow solution is formed,and when $H^{+}$ ions are added to the yellow solution,an orange solution is obtained. Explain why this happens.

What will be the effect of pressure on the equilibrium reaction $C_{(s)} + H_2O_{(g)} \rightleftharpoons H_{2_{(g)}} + CO_{(g)}$?

Le Chatelier's principle is applicable to which of the following?