Question

In a given chemical reaction, the energy of the products is less than the energy of the reactants. Which statement is true for this chemical reaction?

A.Energy is absorbed in the reaction.
B.Energy is released in the reaction.
C.There is no transfer of energy in the reaction.
D.Energy is lost in the reaction.

Answer 1

Energy is released in the reaction

Answer 2

Answer: The correct answer is Option B.

Step-by-step explanation:

Enthalpy change of reaction is defined as the difference in the potential energy of the products and the potential energy of the reactants. It is represented as
`\Delta H_(rxn)`

The equation used to represent enthalpy change of the reaction follows:

`\Delta H_(rxn)=\Delta H_(products)-\Delta H_(reactants)`

• When
  `\Delta H_(rxn)=-ve`, energy is released in the reaction.
• When
  `\Delta H_(rxn)=+ve`, energy is absorbed in the reaction.

As, energy of products is less than the energy of reactants, so the enthalpy change of the reaction comes out to be negative.

Thus, the correct answer is Option B.