The reaction $C_2H_{6(g)} \rightleftharpoons C_2H_{4(g)} + H_{2(g)}$ is at equilibrium in a closed vessel at $1000 \ K$. The enthalpy change $(\Delta H)$ for the reaction is $137.0 \ kJ \ mol^{-1}$. Which one of the following actions would shift the equilibrium to the right?

For the reaction $PCl_{5(g)} \rightleftharpoons PCl_{3(g)} + Cl_{2(g)}$,the forward reaction at constant temperature is favoured by

In a vessel containing $SO_3$,$SO_2$,and $O_2$ at equilibrium,some helium gas is introduced so that the total pressure increases while temperature and volume remain constant. According to Le Chatelier's principle,the dissociation of $SO_3$:

According to Le Chatelier's principle,if a gaseous mixture is compressed,what will be the effect on the equilibrium of the following reaction: $N_2O_{4(g)} \rightleftharpoons 2NO_{2(g)}$?

In the equilibrium reaction
$AgCl_{(s)} + 2NH_3(aq.) \rightleftharpoons [Ag(NH_3)_2]^+ (aq.) + Cl^{-} (aq.)$
Increase in the concentration of $Cl^{-} (aq.)$ causes

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