Exothermic and Endothermic Reactions

The endothermic process is a term that describes a reaction where the system absorbs the energy from its surrounding in the form of heat.
A few examples of the endothermic process are photosynthesis, evaporating liquids, melting ice, dry ice, alkane cracking, thermal decomposition, ammonium chloride in water and much more. * As the name implies, ‘endo’ means ‘to absorb,’ and ‘thermic’ means ‘heat.’
This energy is produced as a result of the reaction of reactants into the product.
It occurs as a result of the dissociation of the bonds between the molecules. * The energy is then released through the formation of new bonds.
Heat is taken up from the surroundings in such reactions, so the temperature of the system where the reaction is taking place remains cooler.
Also, at the end of the reaction, the enthalpy, which is the change in heat energy during the conversion of reactants to products, increases.

The exothermic reaction is the opposite of an endothermic reaction.
It releases energy by light or heat to its surrounding. * A few examples are neutralisation, burning a substance, reactions of fuels, deposition of dry ice, respiration, solution of sulphuric acid into water and much more.
The energy released is caused by the formation of new bonds (products) at a higher level. While the energy required to break up the bonds (reactants) is lower.
At the end of the reaction, the enthalpy change decreases as well. * During chemical reactions, a great deal of energy is required.
This energy was used to maintain the bond that held the molecules together. * As a result of the reactions between molecules and compounds, as well as the breaking of bonds, a tremendous amount of energy is released.