Hess’s Law

Learning Objective

• Employ Hess’s law to determine ΔH∘rxn

Key Points

• Hess’s law states that the standard reaction enthalpy is the sum of the standard enthalpies of the intermediate reactions into which the overall reaction can be divided, while each occurs at the same temperature.
• Enthalpy change for a reaction is independent of the number of ways a product can be obtained, if the initial and final conditions are the same.
• Negative enthalpy change for a reaction indicates exothermic process, while positive enthalpy change corresponds to endothermic process.

Terms

• Hess’s lawStates that, if an overall reaction takes place in several steps, its standard reaction enthalpy is the sum of the standard enthalpies of the intermediate reactions, at the same temperature.
• law of conservation of energyStates that the total amount of energy in any isolated system remains constant; energy cannot be created or destroyed, although it can change forms.

Derivation of Hess’s Law

Hess’s law is a relationship in physical chemistry named after Germain Hess, a Swiss-born Russian chemist and physician. This law states that if a reaction takes place in several steps, then the standard reaction enthalpy for the overall reaction is equal to the sum of the standard enthalpies of the intermediate reaction steps, assuming each step takes place at the same temperature.

Hess’s law derives directly from the law of conservation of energy, as well as its expression in the first law of thermodynamics. Since enthalpy is a state function, the change in enthalpy between products and reactants in a chemical system is independent of the pathway taken from the initial to the final state of the system. Hess’s law can be used to determine the overall energy required for a chemical reaction, especially when the reaction can be divided into several intermediate steps that are individually easier to characterize. Negative enthalpy change for a reaction indicates exothermic process, while positive enthalpy change corresponds to endothermic process.

Calculating Standard Enthalpies of Reaction Using Hess’s Law

$C(s)\{{graphite}\}\rightarrow C(s)\{{diamond}\}\quad\quad \Delta H_{rxn}=?$

Turning graphite into diamond requires extremely high temperatures and pressures, and therefore is impractical in a laboratory setting. The change in enthalpy for this reaction cannot be determined experimentally. However, because we know the standard enthalpy change for the oxidation for these two substances, it is possible to calculate the enthalpy change for this reaction using Hess’s law. Our intermediate steps are as follows:

$C(s)\{graphite\}+O_2(g)\rightarrow CO_2(g)\quad\quad \Delta H^\circ=-393.41\;kJ/mol$

$C(s)\{diamond\}+O_2(g)\rightarrow CO_2(g)\quad\quad \Delta H^\circ=-395.40\;kJ/mol$

In order to get these intermediate reactions to add to our net overall reaction, we need to reverse the second step. Keep in mind that when reversing reactions using Hess’s law, the sign of ΔH will change. Sometimes, you will need to multiply a given reaction intermediate through by an integer. In such cases, you need always multiply your ΔH value by that same integer. Restating the first equation and flipping the second equation, we have:

$C(s)\{graphite\}+O_2(g)\rightarrow CO_2(g)\quad\quad \Delta H^\circ=-393.41\;kJ/mol$

$CO_2(g)\rightarrow C(s)\{diamond\}+O_2(g)\quad\quad\Delta H^\circ=+395.40\;kJ/mol$

Adding these equations together, carbon dioxides and oxygens cancel, leaving us only with our net equation. By Hess’s law, we can sum the ΔH values for these intermediate reactions to get our final value, $\Delta H^\circ_{rxn}$.

$C(s)\{graphite\}\rightarrow C(s)\{diamond\}\quad\quad \Delta H^\circ_{rxn}=1.89\;kJ/mol$