ΔH°f (enthalpy) of CuO(s) is -157.3kJ/mol.
A thermodynamic system's enthalpy, which is one of its properties, is calculated by adding the system's internal energy to the product of its pressure and volume. It is a state function that is frequently employed in measurements of chemical, biological, and physical systems at constant pressure, which the sizable surrounding environment conveniently provides.
Because it tells us how much heat is there in a system, enthalpy is significant (energy). Heat is crucial because it allows us to produce useful work. In terms of a chemical process, an enthalpy shift reveals how much enthalpy was gained or lost. Enthalpy is the system's heat energy.
To calculate the enthalpy of the reaction
ΔH° [tex]_{rxn}[/tex] = ∑nΔH°[tex]_{product}[/tex] - ∑nΔH°[tex]_{reactant}[/tex]
-146.0kJ = (2mol)(ΔH°f of CuO) - (1mol)(-168.6kJ/mol)
-146.0kJ = (2mol)(ΔH°f of CuO) + 168.6kJ/mol
ΔH°f of CuO = [tex]\frac{-146.0kJ - 168.6kJ}{2mol}[/tex]
ΔH°f of CuO = -157.3kJ/mol
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