Question

During a reaction, ΔH for reactants is −750 kJ/mol and ΔH for products is 920 kJ/mol. Which statement is correct about the reaction?

Group of answer choices

It is endothermic because the energy required to break bonds in the reactants is less than the energy released when the products are formed.

It is endothermic because the energy required to break bonds in the reactants is greater than the energy released when the products are formed.

It is exothermic because the energy required to break bonds in the reactants is less than the energy released when the products are formed.

It is exothermic because the energy required to break bonds in the reactants is greater than the energy released when the products are formed.

Answer 1

The reaction is exothermic because the energy required to break bonds in the reactants is less than the energy released when the products are formed. The correct answer is option 3.

Step-by-step explanation:

The reaction is exothermic because the energy required to break bonds in the reactants is less than the energy released when the products are formed.

The enthalpy change (ΔH) of the reaction is approximately -111 kcal/mol, indicating that the reaction releases more energy than it absorbs.

Therefore, the correct statement is: It is exothermic because the energy required to break bonds in the reactants is less than the energy released when the products are formed.