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Enthalpy (H) is a measure of the energy in a system, and the change in enthalpy is denoted by $\Delta H$. Since enthalpy is a state function, the value of $\Delta H$ is independent of the path taken by the reactions to reach the products. Values of $\Delta H$ can be determined experimentally under standard conditions.
The sign of the $\Delta H$ value indicates whether or not the system is endothermic or exothermic. In an endothermic system, the $\Delta H$ value is positive, so the reaction absorbs heat into the system. The equation takes the form:
$heat+A+B\rightarrow C,\;\Delta H=+$
Notice that in an endothermic reaction like the one depicted above, we can think of heat as being a reactant, just like A and B.
Thermochemical Equations for Exothermic Reactions
In an exothermic system, the $\Delta H$ value is negative, so heat is given off by the reaction. The equation takes the form:
$A + B \rightarrow C + heat,\: \Delta H = -$
Notice that here, we can think of heat as being a product in the reaction.
$\Delta H$ is dependent on both the phase (solid, liquid, or gas) as well as the molar ratios of the reactants and products. Therefore, all thermochemical equations must be stoichiometrically balanced. This becomes important once we begin working with Hess's law.
Thermochemical equations can describe endothermic or exothermic reactions.
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The reaction is exothermic; the value of ΔH depends on reactant and product concentration., The reaction is endothermic; the value of ΔH does not depend on reactant and product concentration., The reaction is exothermic; the value of ΔH does not depend on reactant and product concentration., and The reaction is endothermic; the value of ΔH depends on reactant and product concentration.