Question

During an endothermic reaction, Δ H for the reactants was −600 kJ/mol. Which of the following statements is correct about the Δ H for the products? aIt is less than −600 kJ/mol because the amount of energy required to break bonds is less than the amount of energy released in forming bonds. bIt is less than −600 kJ/mol because the amount of energy required to break bonds is greater than the amount of energy released in forming bonds. cIt is greater than −600 kJ/mol because the amount of energy required to break bonds is less than the amount of energy released in forming bonds. dIt is greater than −600 kJ/mol because the amount of energy required to break bonds is greater than the amount of energy released in forming bonds.

Answer 1

So,

In an endothermic reaction, the reaction requires a determined amount of energy to occurs.

The reaction of the problem has H = -600kJ/mol. The reaction is endothermic and the energy that the reaction needs is absorbed by the reactants. That means, the energy of products. Then, the correct answer is:

It is greater than -600kJ/mol because the amount of energy required to break bonds is greater than the amount of energy released in forming bonds.