Answer: Option (2) is the correct answer.
Explanation:
The minimum amount of energy required by the reactants to undergo a reaction is known as activation energy.
And when we add a catalyst into a reaction then it leads to a decrease in activation energy. As a result, product formation becomes faster.
Therefore, we can conclude that intervals 1 and 3 are affected by the addition of a catalyst.
Intervals 1 and 3 are most affected by the addition of catalyst. Option 2 is correct.
Catalysts are those compounds that reduce the activation energy for the reaction to occur, hence increasing the rate of reaction.
Activation energy is the energy that is required to start a reaction. Here, 1 represents the activation energy and 3 represents activation energy without catalyst.
Therefore, intervals 1 and 3 are most affected by the addition of catalyst.
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