The reaction $2SO_2 + O_2 \rightleftharpoons 2SO_3$; $\Delta H = -ve$ is favoured by

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

The binding of oxygen by haemoglobin $(Hb)$ forming $(HbO_2)$ is partially regulated by the concentration of $H_3O^{+}$ and dissolved $CO_2$ in blood.
$HbO_2 + H_3O^{+} + CO_2 \rightleftharpoons (H^{+} - Hb - CO_2) + O_2 + H_2O$
Release of $O_2$ is favoured when there is:

What happens when an inert gas is added at constant pressure to a reversible decomposition reaction that is in equilibrium?

The formation of ammonia from its constituent elements is an exothermic reaction. The effect of increasing temperature on the reaction equilibrium is

For a given equilibrium reaction,addition of inert argon gas at constant volume can shift the equilibrium in $N_{2(g)} + 3H_{2(g)} \rightleftharpoons 2NH_{3(g)}$