Question

The minimum amount of energy that requires to start a chemical reaction ​

Answer 1

Answer:

The minimum amount of energy needed for a reaction to proceed is the least amount of kinetic energy which molecules must have to cause an “effective collision” (i.e. a collision which can break pre-existing bonds), this is also known as the Activation Energy of a chemical reaction.

Explanation:

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Answer 2

Answer:

The minimum amount of energy needed for a reaction to proceed is the least amount of kinetic energy which molecules must have to cause an “effective collision” (i.e. a collision which can break pre-existing bonds), this is also known as the Activation Energy of a chemical reaction.

Explanation:

Collision Theory is often used to explain the rate at which a chemical reaction proceeds. Simply, for a reaction to occur, molecules must collide with sufficient energy (as well as at the right orientation). The minimum amount of energy needed for a reaction to proceed is the least amount of kinetic energy which molecules must have to cause an “effective collision” (i.e. a collision which can break pre-existing bonds), this is also known as the Activation Energy of a chemical reaction.

The activation energy for a specific reaction changes depending on a number of factors such as concentration of reactants, temperature, nature of reactants, particle size and can also be affected by the use of a catalyst.

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