Question

The activation energy of a reaction going on its own is 20 kj. If the reaction was treated with a catalyst, which would most likely represent the amount of energy needed to start a reaction?

15 kj
20 kj
25 kj
30kj

Answer 1

A 15kj

Step-by-step explanation:

just did the assignment

Answer 2

15 kJ

Step-by-step explanation:

We need to know the following;

what is activation energy?

• Activation energy is the minimum energy required by reactants for a chemical reaction to take place.

What are catalysts?

• Catalysts are molecules or substances that speed up the rate of a chemical reaction.

• In other words, catalysts increase the speed at which products are formed from reactants.

How do catalysts speed up reactions?

• Catalysts speed the rate of chemical reactions by lowering the activation energy of the reactants.
• When activation energy is lowered, reactants require less energy for the reaction to occur which easily achieved making the reaction proceed faster.
• Therefore, in presence of a catalyst, the new activation energy should be lower than the initial value of activation energy.