The statement, that describes the reaction and correctly compares the energy in bonds from the given ΔH values is "It's endothermic because the energy required to break bonds in the reactants is less than the energy released when the products are formed."
What is ΔH?
The quantity of energy evolved during a chemical reaction is represented by ΔH, also known as enthalpy change.
An exothermic reaction is a chemical reaction in which heat energy is emitted. The value of ΔH is always negative in exothermic processes. An endothermic reaction is a chemical reaction that absorbs heat energy. The value ΔH of is always positive for endothermic reactions.
When the bonds in the reactants are broken, more energy is absorbed than is released when new bonds are created in the products, therefore the value of ΔH is always positive in endothermic reactions.
Hence the correct option is endothermic because the energy required to break bonds in the reactants is less than the energy released when the products are formed.
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