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Germain Henri Hess studied heat changes accompanying chemical reactions. Hess's law expresses the additivity of compatible reaction enthalpies: reversing a reaction reverses the sign, and combining reaction equations combines their enthalpy changes. This makes it possible to obtain an otherwise inaccessible heat change from an enthalpy cycle.^[ref]

A chemist who studied energy changes during chemical reactions; Hess's law bears his name.

Royal Society of Chemistry biographical notice: edu.rsc.org/resources/on-this-day-aug-08--henri-hess-was-born/10808.article

Hess's law states that compatible chemical reaction enthalpies add when their equations add. Reversing a chemical reaction reverses its enthalpy change; multiplying the entire chemical reaction equation by a factor multiplies that change by the same factor. The reason is that enthalpy is a state function: intermediate states cancel from the differences. A cycle supplies one independent balance relation; it cannot determine two unknown inputs without further information.

The law is named after Germain Henri Hess.

For specified initial and final thermodynamic states, the change is $\Delta H=H_{\mathrm{final}}-H_{\mathrm{initial}}$. Because enthalpy is an extensive variable, a quoted reaction $\Delta H$ belongs to the amount of substance specified for each species in its chemical equation. Reversing the equation changes the sign; scaling every coefficient scales $\Delta H$; adding compatible equations adds their $\Delta H$ values. A per-mole value must say which chemical equation and normalization it uses. Match temperature, pressure, thermodynamic phases, chemical solution compositions and reference states before cancellation; the same formula in a gas and a liquid represents different states.^[ref]

The value of Hess's law is that an inaccessible reaction enthalpy can be obtained from measurable transformations. The algebra does not require those transformations to be steps of the actual reaction mechanism. Neither an activation energy nor a reaction rate follows from the endpoint difference: a catalyst may change the reaction rate while preserving the compatible initial and final enthalpies.

Klaus Theopold coauthored an introductory treatment connecting chemical equations with energy balances. The enthalpy chapter explains why reversing a reaction reverses its heat-change sign and why compatible equations can be combined through Hess's law.^[ref]

Paul Flowers coauthored an introductory chemistry text that develops quantitative thermochemistry. Its treatment of Hess's law keeps the reaction equation attached to the stated enthalpy change, so changing the amount reacted changes the corresponding energy.^[ref]

Richard Langley coauthored an introductory account of chemical thermodynamics. Its enthalpy examples show how measurements of accessible reactions can be combined to obtain an otherwise inaccessible reaction's energy change using Hess's law.^[ref]

William R. Robinson coauthored an introductory chemistry text whose thermochemistry chapter develops Hess's law. Adding compatible reaction equations cancels intermediates and adds their enthalpy changes, connecting symbolic chemical bookkeeping with measurable heat.^[ref]