Question

Which one of the following is not a correct equation for enthalpy of formation? (Products are correct)

a. ΔH°f = ΣΔH°f(products) - ΣΔH°f reactants
b. ΔH°f = ΣΔH°f reactants - ΣΔH°f(products)
c. ΔH°f = ΣΔH°f(products) + ΣΔH°f reactants
d. ΔH°f = ΣΔH°f reactants + ΣΔH°f(products)

Answer 1

The correct equation for enthalpy of formation is ΔH°f = ΣΔH°f(products) - ΣΔH°f(reactants).

Step-by-step explanation:

The correct equation for enthalpy of formation is:

ΔH°f = ΣΔH°f(products) - ΣΔH°f(reactants)

In this equation, the enthalpies of formation for the products are subtracted from the enthalpies of formation for the reactants. This equation follows the principle of Hess's Law, which states that the enthalpy change of a reaction is equal to the sum of the enthalpies of formation of the products minus the sum of the enthalpies of formation of the reactants.