The equation indicates that $\text{H}_2(g)$ and $\text{I}_2(g)$ combine to establish an equilibrium mixture. $\text{H}_2(g) + \text{I}_2(g) \rightleftharpoons 2\text{HI}(g)\qquad \Delta H^{\circ} = -9.6\,\text{kJ mol}^{-1}$ An equal-amount mixture of $\text{H}_2(g)$ and $\text{I}_2(g)$ is prepared at temperature $T_1$, and the mixture’s composition is followed. The outcome is shown on a graph. The experiment is carried out again at a lower temperature, $T_2$. Which new graph would be obtained?