Final answer:
The statement is true; an exothermic reaction in an adiabatic container results in products being at a higher temperature than the reactants due to the increase in internal energy of the system.
Step-by-step explanation:
The question is assessing the thermal outcomes of a chemical reaction taking place in an adiabatic container. In an adiabatic container, no heat is exchanged with the surroundings, and thus, if an exothermic reaction occurs, the energy released increases the internal energy of the system. Since an exothermic reaction results in the release of heat (ΔH < 0), and the reaction we are discussing also has a positive entropy change (ΔS > 0), this leads to a spontaneous reaction (ΔG < 0) at all temperatures. Therefore, the statement that the products in an exothermic reaction carried out in an adiabatic container are at a higher temperature than the reactants is true.
When a substance gains thermal energy, its temperature increases (ΔT >0), which is the case in an exothermic reaction in an adiabatic setup. Moreover, the temperature for Gibbs free energy is always measured in Kelvin, indicating that it can only be positive; when ΔH is negative and ΔS is positive, it reinforces the outcome that the products will indeed be at a higher temperature than the reactants.