Delta H of reaction (ΔHr) is the change in enthalpy of a chemical reaction, which is a measure of the energy released or absorbed during the reaction. It is also known as the heat of reaction.
Bond energies are the amount of energy required to break a particular type of bond between two atoms in a molecule. They are measured in units of kilojoules per mole (kJ/mol).
The formula for calculating delta H of reaction using bond energies is: ΔHr = ∑(bond energies of bonds broken) - ∑(bond energies of bonds formed). This means you add up the bond energies of all the bonds broken in the reactants and subtract the bond energies of all the bonds formed in the products.
Calculating delta H of reaction using bond energies is useful because it provides a way to estimate the energy released or absorbed during a chemical reaction. It can also help predict the stability of a molecule and its reactivity.
There are a few limitations to using bond energies to calculate delta H of reaction. One limitation is that it assumes all bonds in the reactants and products are broken or formed simultaneously, which is not always the case. It also does not account for any changes in bond lengths or bond angles during the reaction. Additionally, bond energies are average values and may not accurately represent the specific bonds in a particular molecule.
