What is the value of the activation energy of the uncatalyzed reaction? express your answer to three significant figures and include the appropriate units.

175KJ

Explanation:

I will assume the diagram is as in the attachment I’ve supplied herein.

Activation energy is the minimum energy required by reactant particles for a chemical reaction to occur. Depending on reaction conditions, especially for reversible reactions, reactants can become products and vice versa.

Activation energy for a forward reaction = energy of the activated complex (transition state) – energy of the reactants.

Activation energy for a reverse reaction = energy of the activated complex – energy of the products.

For the forward reaction above, reading the values from the diagram,

Activation energy = energy of the activated complex –energy of the reactants

Activation energy = (400 – 225)KJ = 175KJ

i think it is true since you can test the answer and can use observations to complete it.