Question

In an exorthermic reaction, what is the relation between the energy stored in the reactants to the energy stored in the products?

Answer 1

In an exothermic reaction, heat is released. ΔH for an exothermic reaction is negative. That means that the energy stored in the reactants is higher than the energy stored in the products. 

The opposite is true for an endothermic reaction. Heat is absorbed, and ΔH for an endothermic reaction is positive. This means that energy stored in the products is higher than the energy stored in the reactants.

Answer 2

Explanation:

Exothermic reactions are defined as the reactions in which energy of reactants is more than the energy of the products.

In these reactions, energy is released by the system. The total enthalpy of the reaction $(\Delta H)$ comes out to be negative.

Energy of reactants are higher than energy of products.

$\Delta H_{reactant}>\Delta H_{product}$

$\Delta H=\Delta H_{product}-\Delta H_{reactant}$