H3PO4(aq) + H2O(l) ↔ H2PO4-(aq) + H3O+(aq) ΔH = -13kJ at 298K In the reaction above, an increase in temperature would

Answer Details

The given chemical equation is a reversible exothermic reaction, and the value of enthalpy change, ΔH, is negative. According to Le Chatelier's principle, an increase in temperature will favor the endothermic reaction to absorb heat and therefore, will shift the equilibrium towards the reactants' side. Thus, an increase in temperature would favor the reverse reaction. Hence, the correct option is: "favor the reverse reaction."