Related Questions
What is the difference between a catalyzed and uncatalyzed reaction?The uncatalyzed reaction proceeds via a one-step mechanism (one transition state observed), whereas the catalyzed reaction follows a two-step mechanism (two transition states observed) with a notably lesser activation energy.
What is the activation energy for the uncatalyzed reaction?The activation energy of an uncatalyzed reaction is 91 kJ/mol . The addition of a catalyst lowers the activation energy to 46 kJ/mol .
What does a catalyst do to the required activation energy as compared to a uncatalyzed reaction pathway How do you think this affects the reaction rate?A catalyst lowers the activation energy by changing the transition state of the reaction. The reaction then goes through a different pathway/mechanism than the uncatalyzed reaction. The catalyst does not change the net energy difference between reactant and product.
Why might the activation energy be lower in the catalyzed reaction than the uncatalyzed reaction?Catalysts participate in a chemical reaction and increase its rate. They do not appear in the reaction's net equation and are not consumed during the reaction. Catalysts allow a reaction to proceed via a pathway that has a lower activation energy than the uncatalyzed reaction.
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