Thermochemistry

Thermochemistry is the application of thermodynamics to chemistry.

Thermochemistry is used to predict the button exchanges that occur in the following processes:

1.         chemical reactions

2.         phase changes such as simmering and melting

3.         the organic law of responses

Thermochemistry is primarily concerned with the following state functions delineate in thermodynamics:

        Internal energy (U)

        Enthalpy (H).

        Entropy (S)

        Gibbs light energy (G)

Most identities in Thermochemistry arise from application of the first legal philosophy of thermodynamics, the Law of Conservation of Energy, to these state function.

In chemical reactions, bonds are broken in and reformed, and passionateness may be given off or taken up in such processes. Since reactions are frequently carried out at constant pressure, the change in total heat is the appropriate measure of heat given off or absorbed.

Laws of Thermochemistry

1.         The magnitude of H is directly proportional to the amount of reactant or product.

-Thus H can be used as a conversion factor in a balanced equivalence to obtain amounts of reactant/product or H itself. ( gram molecule to mole ratios).

2.          H for a reaction is equal in magnitude moreover opposite in sign to H for the reverse reaction.

Heats of Formation

Molar heat of formation ( Hf) is equal to the enthalpy change, H when one mole of the compound is formed from the elements in their stable forms at 25oC and 1 atm is Ho (pronounced delta h naught). Ho of a solution is of a 1M solution, at 1 atm and 25 oC.

Heats of formation are usually negative quantities.

Heat is a way of transferring energy between a system and its surroundings that often, but not always, changes the temperature of the system. Heat is not conserved, it can be either created or destroyed. In the metric system, heat is measured in units of calories,

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