# Enthalpy change and equilibrium

I don't understand why enthalpy change won't change at an equilibrium?

The reason I ask this is because of this question:

At first I thought the answer is C, but I realised that the amount depends on where the position of equilibrium lies. The correct answer is D, but doesn't enthalpy change (delta H) also depend on where the position of equilibrium lies?

• (C) can be incorrect as amount might refer to mass formed, which won't be the same at all. Dec 31 '15 at 8:28
• Trick questions. (D) is correct since the equilibrium position is reversed as the reaction itself is reversed, so the enthalpy change is also reversed (by your own logic). Dec 31 '15 at 8:30
• @TamoghnaChowdhury, in chemistry the word amount refers to number of moles, not mass. C would be correct only if the system were to begin with reactants and no products, so it is not always true, as stipulated by the question. Oct 29 '21 at 13:02
• @Rafael while your first point is likely to be correct (depending on textbook localizations and whatnot), the second is unnecessarily contrived - equilibrium implies no net progress of the equation in either direction, microscopic transient fluctuations in the amounts of the reactants and products can always occur. Nov 7 '21 at 23:18

The answer to this question is related to the definition of $\Delta H^0$. It is precisely defined as the enthalpy change between the following two thermodynamic equilibrium states: