Question

When a given reaction is conducted in a calorimeter, energy is absorbed from the surrounding water and results in a decrease in the water’s temperature. Which of the following best describes the difference in the potential energy of the reactants and products in this reaction?

The potential energy remains low before and after the reaction.
The potential energy of the reactants is higher than that of the products.
The potential energy of the reactants is much lower than that of the products
The potential energy of the reactants does not differ from that of the products.

Answer 1

The potential energy of the products is higher than the potential energy of the reactants.

Answer 2

Answer: The potential energy of the reactants is much lower than that of the products

Explanation: Endothermic reactions are defined as the reactions in which energy of the product is greater than the energy of the reactants. The total energy is absorbed in the form of heat and $\Delta H$ for the reaction comes out to be positive.

Exothermic reactions are defined as the reactions in which energy of the product is lesser than the energy of the reactants. The total energy is released in the form of heat and $\Delta H$ for the reaction comes out to be negative.

Thus as the reactants have absorbed energy from the surrounding water, the energy of the products will be higher and the reaction is termed as endothermic reaction.