On addition of an inert gas at constant volume to the reaction $N_2 + 3H_2 \rightleftharpoons 2NH_3$ at equilibrium,

For an exothermic reaction,the equilibrium constant:

$N_2$ and $O_2$ combine to form nitric oxide as follows: ${N_2}_{(g)} + {O_2}_{(g)} \rightleftharpoons 2NO - \text{heat}$. Which of the following conditions will favor the production of $NO$?

In which of the following systems will doubling the volume of the container cause a shift to the right?

Does the number of moles of reaction products increase,decrease,or remain the same when each of the following equilibria is subjected to a decrease in pressure by increasing the volume?
$(a) \quad PCl_{5(g)} \longleftrightarrow PCl_{3(g)} + Cl_{2(g)}$
$(b) \quad CaO_{(s)} + CO_{2(g)} \longleftrightarrow CaCO_{3(s)}$
$(c) \quad 3Fe_{(s)} + 4H_2O_{(g)} \longleftrightarrow Fe_3O_{4(s)} + 4H_{2(g)}$

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: