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

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

catalyst works by lowering the activation energy required for a reaction to proceed. Therefore, if the original activation energy of the reaction is 20 kJ and the reaction is treated with a catalyst, the amount of energy needed to start the reaction would likely be less than 20 kJ.Among the given options, 15 kJ is the only value that is lower than 20 kJ. Thus, the most likely amount of energy needed to start the reaction with a catalyst would be:15 kJ

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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

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