Some inert gas is added at constant volume to the following reaction at equilibrium:
$NH_4HS_{(s)} \rightleftharpoons NH_{3(g)} + H_2S_{(g)}$
Predict the effect of adding the inert gas.

Which of the following equilibria will shift to the right side on increasing the temperature?

The reaction $A + B \rightleftharpoons C + D + \text{heat}$ has reached equilibrium. The reaction may be made to proceed forward by:

What is true for the equilibrium reaction? $CH_3COOH + CH_3OH \rightleftharpoons[cat.]{} CH_3COOCH_3 + H_2O$

In which of the following reactions at equilibrium,the position of the equilibrium shifts towards the products,if the total pressure is increased?
$(I)$ $X_{2(g)} + 3Y_{2(g)} \rightleftharpoons 2XY_{3(g)}$
$(II)$ $X_{2(g)} + Y_{2(g)} \rightleftharpoons 2XY_{(g)}$
$(III)$ $X_{2(g)} + Z_{2(g)} \rightleftharpoons 2XZ_{(g)}$
$(IV)$ $X_{2(g)} + Y_{4(g)} \rightleftharpoons 2XY_{2(g)}$

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