Exothermic reaction

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In chemistry, an exothermic reaction is one that releases heat . It is the opposite of an endothermic reaction. Expressed in a chemical equation:

<math>reactants \rightarrow \; product + energy</math>

1 Overview
2 Examples of exothermic reactions
3 Key points
4 See also
5 External links

[edit] Overview

In an exothermic reaction, the total energy absorbed in bond breaking is less than the total energy released in bond making.

When using a calorimeter, the change in heat of the calorimeter is equal to the opposite of the change in heat of the system. This means that when the medium in which the reaction is taking place gains heat, the reaction is exothermic.

The absolute amount of energy in a chemical system is extremely difficult to measure or calculate. The enthalpy change, ΔH, of a chemical reaction is much easier to measure and calculate. A bomb calorimeter is very suitable for measuring the energy change, ΔH, of a combustion reaction. Measured and calculated ΔH values are related to bond energies by:

<math>\Delta \;\!\!H = energy\;used\;in\;bond\;breaking\;reactions - energy\;released\;in\;bond\;making\;products</math>.

by definition the enthalpy change has a negative value:

<math>\Delta\;\!\!H < 0 </math>

For an exothermic reaction, this gives a negative value for ΔH, since a larger value (the energy released in the reaction) is subtracted from a smaller value (the energy used for the reaction). For example, when hydrogen burns:

<math>2H_2 + O_2 \rightarrow \; 2H_2O</math>

<math>\Delta\;\!\!H = -483.6\ kJ/mol\ of\ O_2</math>

[edit] Examples of exothermic reactions

Combustion reactions
Neutralization reactions for instance direct reaction of acid and base
Adding concentrated acid to water
Adding water to anhydrous copper(II) sulfate
The Thermite reaction
Reactions taking place in a self-heating can based on lime and aluminum.

[edit] Key points

The concepts exothermic and its opposite number endothermic relate to the enthalpy change in any process not just chemical reaction
In endergonic reactions and exergonic reactions it is the sign of the Gibbs free energy that count and not enthalpy. the related concepts endergonic and exergonic apply to all physical processes.
the conceptually related endotherm and exotherm are concepts in Animal physiology.