Answer: Option (d) is the correct answer.
Explanation:
Activation energy is the minimum energy required by the reactants to undergo a specified reaction.
When there is increase in activation energy then energy barrier will also increase therefore, reactant molecules will less energy cannot cross the energy barrier.
As a result, they will not participate in the reaction and hence, there will be decrease in rate of reaction.
Thus, we can conclude that the reaction begins to slow down as the activation energy increases.
The rate of the reaction depends on the activation energy and is inversely proportional. As the activation energy increases the reaction rate or speed decreases. Thus, option D is correct.
The speed at which the reactants undergo changes to form the products is called the rate of reaction. The rate of the product formation depends on the activation energy, temperature, catalysts, etc.
The activation energy is required by the reactant to cross the barrier to form the product and inversely affects the reaction rate. Increased activation hinders the collision of the particles.
The decreased collision reduces the kinetic energy of the molecules to undergo chemical changes to yield product. As a result, the reaction slows down.
Therefore, in option D. the activation energy reduces the chemical reaction.
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