Laplace number

The standard enthalpy of reaction (denoted Δ_rH^⊖) is the enthalpy change that occurs in a system when one mole of matter is transformed by a chemical reaction under standard conditions.

For a generic chemical reaction

−v_A A + −v_B B + ... → v_P P + v_Q Q ...

the standard enthalpy of reaction ΔH_r^⊖ is related to the standard enthalpy of formation ΔH_f^o of the reactants and products by the following equation:

$\mathrm{\Delta }{H}_{\mathrm{r}}^{\ominus }=\sum _B{v}_B\mathrm{\Delta }{H}_{\mathrm{f}}^{\ominus }(B)$

In this equation, v_B is the stoichiometric number of entity B.

A similar enthalpy change is the standard enthalpy of formation, which has been determined for a vast number of substances. The enthalpy change of any reaction under any conditions can be computed, given the standard enthalpy of formation of the reactants and products.

It is defined as the amount of heat absorbed or evolved in the transformation of the reactants at a given temperature and pressure into the products at the same temperature and pressure. Enthalpy of a reaction at constant pressure and at a constant volume: Enthalpy of a reaction depends upon the conditions under which the reaction is carried out. There are two general conditions under which Thermochemical measurements are made.

(a) Constant volume (b) Constant pressure

The magnitudes of the enthalpy changes in these two conditions are different. In first case the volume of the system is kept constant during the course of the measurement by carrying out the reaction in a closed and rigid container and as there is no change in the volume and so no work is also involved.

From the first law of thermodynamics we have a relation, $\mathrm{\Delta }E=Q_v$

That is, the enthalpy of a reaction at constant volume is equal to the change in the internal energy (Δ E) of the reacting system.

The thermal change that occurs in a chemical reaction is only due the difference in the sum of internal energy of the products and the sum of the internal energy of reactants.

$\mathrm{\Delta }E=\sum E_{products}-\sum E_{reactants}$

This also signifies that the amount of heat absorbed at constant volume could be identified with the change in the thermodynamic quantity.

At constant pressure, the system is either kept open to the atmosphere or confined within a container on which a constant external pressure is exerted and under these conditions the volume of the system changes. The thermal change at a constant pressure not only involves the change in the internal energy of the system but also the work performed either in expansion or contraction of the system.

$Q_p=\mathrm{\Delta }E+W$ (work)

If ‘W’ is only pressure – volume work, then we have

$Q_p=\mathrm{\Delta }H=\mathrm{\Delta }E+P\mathrm{\Delta }V$

$Q_p=(\sum E_p-\sum E_r)+P(V_p-V_r)$

$Q_p=(\sum E_p+P{V}_p)-(\sum E_r+P{V}_r)$

As enthalpy or heat content is defined by $H=E+PV$. So we have, $Q_p=\sum H_p-\sum H_r=\mathrm{\Delta }H$ At constant pressure, the heat of the reaction is exactly equal to the enthalpy change, $\mathrm{\Delta }H$, of the reacting system.