In the $N_2 + 3H_2 \rightleftharpoons 2NH_3$ reversible reaction,an increase in pressure will favour:

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

Which of the following conditions is favorable for the forward reaction in the equilibrium: $H_2 \rightleftharpoons H + H$ $(\Delta H = +ve)$?

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

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?

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