Standard Enthalpies of Formation, ΔH°f

The quantity of energy associated with the formation of one mole of a substance from its elements (in their standard states).

The standard states (at SATP) of most elements are solid, except for the gaseous diatomic molecules, H₂, O₂, N₂, F₂, Cl₂, and the two liquid elements Hg and Br₂.

These energies can be looked up in standard tables and have the units, KJ/mol.

Writing Formation Reactions:

• Write one mole of the product in the state that has been specified on the product side.
• Write the reactant elements in their standard states
• Balance the equation for only one mole of product.

For example:

Write the formation reaction for glucose, C₆H₁₂O_6(s).

C_(s) +     H_2(g) +   O_2(g) ->     C₆H₁₂O_6(s) ΔH°_f = -1273.1KJ/mol

Now, balance the equation for one mole of glucose produced.

6C_(s) +     6H_2(g) +   3O_2(g) ->     C₆H₁₂O_6(s)

The standard state for elements in their standard states is zero.

For example;

Br_{2(l) →} Br_2(l) ΔH°_f = 0

The enthalpy change for any equation (target equation) equals the sum of the enthalpies of formation of the products minus the sum of the enthalpies of formation of the reactants.

ΔH  =  ∑nΔH°_f(products) –  ∑nΔH°_f(reactants)

Note:  Each of the product and reactants is multiplied by the number of moles of each in the equation (target equation).

William Anderson (Schoolworkhelper Editorial Team)

William completed his Bachelor of Science and Master of Arts in 2013. He current serves as a lecturer, tutor and freelance writer. In his spare time, he enjoys reading, walking his dog and parasailing. Article last reviewed: 2022 | St. Rosemary Institution © 2010-2024 | Creative Commons 4.0

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