To determine the conditions that favor maximum formation of the product in the reaction$\\ A_2(g) + B_2(g) \rightleftharpoons X_2(g), \Delta_r H = -X$ kJ$,$ we need to consider both$\\$Le Chatelier's principle and the effect of temperature and pressure on equilibrium.$\\$1. Effect of Temperature:$\\$• The reaction is exothermic, as indicated by the negative $\Delta_r H. \\$• According to Le Chatelier's principle, decreasing the temperature will favor the$\\$ formation of products in an exothermic reaction.$\\$2. Effect of Pressure:$\\$• The reaction involves 2 moles of gaseous reactants (A$_2$ and B$_2)$ and 1 mole of$\\$ gaseous product (X$_2). \\$• Increasing the pressure will favor the side with fewer moles of gas, which is the$\\$ product side in this case.$\\$Combining these effects, the conditions that favor maximum formation of the product$\\$are low temperature and high pressure.$\\$Therefore, the correct option is:$\\$Option 3: Low temperature and high pressure.