Why is the reactant in endothermic reaction stronger than the product?

[Sophie Zhou 2H]

As the subject says, why is the reactant in endothermic reaction stronger than product? I understand that from the equation of calculating enthalpy change= enthalpy of bonds broken-enthalpy of bonds formed. It does reflect that the bond enthalpy of reactants is larger, thus, the reactant is stronger.

But from the energy diagram, isn't the product higher than the reactant? Why is that and is the energy diagram y-axis not representing the bond enthalpies?

[406477008]

Hello, the reaction in endothermic reactions have a stronger bond therefore the reaction is stronger. I hope this helps!

[sihupark]

Reactants have stronger bonds than products as more energy is required to break their bonds, which is why they are placed lower on the energy diagram. It is also important to note that the energy diagram shows total enthalpy and not bond enthalpy. The products appear higher because the system absorbs energy, making the total enthalpy of the products greater than that of the reactants. This doesn't mean that the reactants don't have stronger bonds than products, but rather shows the net energy change in the reaction.