Exothermic reaction

Exothermic reaction

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Exothermic reaction

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

reactants ? product + energy

Overview
Examples of exothermic reactions
Key points
Measurement
See also
External links

Overview

In an exothermic reaction, the total energy absorbed in bond breaking is less than the total energy released in bond making. In other words, the energy needed for the reaction to occur is less than the total energy provided. As a result of this, the extra energy is released, usually in the form of heat.

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, ?H, of a chemical reaction is much easier to measure and calculate. A bomb calorimeter is very suitable for measuring the energy change, ?H, of a combustion reaction. Measured and calculated ?H values are related to bond energies by:

?H = energy used in bond breaking reactions - energy released in bond making products

A sketch of an exothermic reaction

by definition the enthalpy change has a negative value:

?H < 0

For an exothermic reaction, this gives a negative value for ?H, 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:

2H₂ + O₂ ? 2H₂O

?H = -483.6 kJ/mol of O₂

Examples of exothermic reactions

A thermite reaction using Iron(III) Oxide

Combustion reactions of fuels
Neutralization reactions such as 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 aluminium
The setting of cement and concrete
Many corrosion reactions such as oxidation of metals
Most polymerisation reactions
The Haber-Bosch Process of ammonia production

Key points

The concept 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.
In quantum numbers, when any exited energy level goes down to its original level for example: when n=4 fall to n=2, energy is released so, it is exothermic.

Measurement

Heat production or absorption in either a physical process or chemical reaction are measured using calorimetry. One common laboratory instrument is the Differential scanning calorimeter or DSC, where a small sample is slowly heated in a controlled way and the heat flow into or from the sample chamber is monitored. The technique can be used to follow chemical reactions as well as physical processes, such as melting and boiling (both of which are endothermic). Crystallization and condensation, the reverse processes, are both exothermic.