The table shows the thermodynamic data for a reaction. Thermodynamic Data Energy of the Reactants Energy of the Products Activation Energy 160 kJ 370 kJ 260 kJ Which of the following statements explains if the reaction is endothermic or exothermic? The activation energy is lower than the change in enthalpy, so it is an exothermic reaction. The activation energy is higher than the change in enthalpy, so it is an endothermic reaction. The change in enthalpy is - 210 kJ, so it is an exothermic reaction. The change in enthalpy is + 210 kJ, so it is an endothermic reaction.

The change in enthalpy is + 210 kJ, so it is an endothermic reaction.

Explanation:

The change in enthalpy shows that the reaction is exothermic or endothermic.

The change in enthalpy = The energy of products - the energy of reactants.

If ΔH is positive value, the reaction is endothermic, the energy of the products is higher than that of the reactants. If ΔH is negative value, the reaction is exothermic, the energy of the products is lower than that of the reactants.

For this reaction: The change in enthalpy = The energy of products - the energy of reactants = 370 kJ - 160 kJ = + 210 kJ.

So, the right choice is: The change in enthalpy is + 210 kJ, so it is an endothermic reaction.