What conditions must be met in order for a reaction to be considered exothermic?

An exothermic reaction is just where heat is released. So basically if heat is released during the reaction is is an exothermic one.

Answered by TaylorBayley | 2024-06-10

To be considered exothermic, a reaction must satisfy the following conditions:

The reaction releases more energy through the formation of new bonds than the energy required to break the initial bonds.
It involves the transformation of weaker bonds into stronger ones, resulting in a net release of energy.
The reaction often occurs spontaneously under standard thermodynamic conditions, which typically means under a pressure of 1 atmosphere and at a temperature of 25°C.

Additionally, an exothermic reaction can be identified by the fact that its enthalpy change (ΔH) is negative, indicating that heat is given off to the surroundings, raising their temperature. Heat is considered a product of the reaction. Moreover, exothermic reactions might necessitate specific arrangements to manage the heat transfer safely.

Answered by DiBotcher | 2024-06-24

An exothermic reaction releases more energy when new bonds form than is consumed when old bonds break, resulting in a negative enthalpy change. Key conditions include energy release, stronger bonds in products, and a lower energy of products compared to reactants. Common examples include combustion and acid-base reactions.
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Answered by DiBotcher | 2024-12-26