Respuesta :
Reaction B exists likely to happen at a faster rate than reaction A because of its low activation energy.
The statement about reaction A and reaction B exists true.
Therefore, the correct answer is option A. Reaction B exists likely to happen at a faster rate than reaction A.
What is activation energy?
Activation energy can be described as the lowest quantity of energy that must be provided for responding to chemical elements, to experience a chemical reaction. Therefore, the activation energy of a chemical reaction must rather be reached by its combining chemical elements (reactants) before it can begin or form.
As a general practice, the lower the activation energy of a chemical reaction, the more rapid the rate of a chemical reaction, and vice-versa. This eventually implies that the activation energy of a chemical reaction should be diminished, for it to happen fast and sufficiently over a short period of time.
In conclusion, reaction B exists likely to happen at a faster rate than reaction A because of its low activation energy.
Therefore, the correct answer is option A. Reaction B exists likely to happen at a faster rate than reaction A.
To learn more about reactions refer to:
brainly.com/question/537100
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The complete question is:
Reaction A has high activation energy, whereas reaction B has low activation energy. Which of the statements about reaction A and reaction B are true?
A. Reaction B is likely to occur at a faster rate than reaction A.
B. Reaction A is more likely to occur at all than reaction B.
C. Reaction B is more likely to occur at all than reaction A.
D. Reaction A is likely to occur at a faster rate than reaction B.
