Question

Define: a) Reaction intermediate
b) Energy of activation​

Answer 1

Answer:

A reaction intermediate or an intermediate is a molecular entity that is formed from the reactants (or preceding intermediates) and reacts further to give the directly observed products of a chemical reaction. Most chemical reactions are stepwise, that is they take more than one elementary step to complete.

activation energy is the minimum amount of energy that must be provided to compounds to result in a chemical reaction.The activation energy of a reaction is measured in joules per mole, kilojoules per mole or kilocalories per mole.

Explanation:

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Answer 2

Answer:

Reaction intermediate :- >A reaction intermediate or an intermediate is a molecular entity that is formed from the reactants and reacts further to give the directly observed products of a chemical reaction. Most chemical reactions are stepwise, that is they take more than one elementary step to complete.

Energy of activation :- In chemistry and physics, activation energy is the minimum amount of energy that must be provided to compounds to result in a chemical reaction.The activation energy of a reaction is measured in joules per mole, kilojoules per mole or kilocalories per mole.

In short we can define energy of activation :- The energy required to end a chemical reaction. the energy required to bind a substrate to an active site.

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