Which statement below best describes how the catalyst affected the reaction rate shown in this diagram?
This graph shows two potential energy curves of a reaction as it relates to its reaction pathway. One of the curves shows the reaction before a catalyst is used. At the start of this reaction curve, the potential energy of the reactants is low. In the transition state, the potential energy increases rapidly, reaches a peak, then decreases quite rapidly slightly. At the end of the reaction, the potential energy of the products is much lower than at the start of the reaction. The second curve, illustrated with a dashed line, shows the potential energy reaction when a catalyst is used. This potential energy curve starts at the same level as the first, but does not climb as rapidly or as high. Its peak is rather flat. It then drops gradually to the same level as the original potential energy curve.
The addition of the catalyst decreased equilibrium and slowed down the reaction.
The addition of the catalyst increased the temperature of the reactants and sped up the reaction.
The addition of the catalyst decreased the activation energy of the reactants and sped up the reaction.
The addition of the catalyst increased the potential energy of the reactants and slowed the reaction.
This graph shows two potential energy curves of a reaction as it relates to its reaction pathway. One of the curves shows the reaction before a catalyst is used. At the start of this reaction curve, the potential energy of the reactants is low. In the transition state, the potential energy increases rapidly, reaches a peak, then decreases quite rapidly slightly. At the end of the reaction, the potential energy of the products is much lower than at the start of the reaction. The second curve, illustrated with a dashed line, shows the potential energy reaction when a catalyst is used. This potential energy curve starts at the same level as the first, but does not climb as rapidly or as high. Its peak is rather flat. It then drops gradually to the same level as the original potential energy curve.
The addition of the catalyst decreased equilibrium and slowed down the reaction.
The addition of the catalyst increased the temperature of the reactants and sped up the reaction.
The addition of the catalyst decreased the activation energy of the reactants and sped up the reaction.
The addition of the catalyst increased the potential energy of the reactants and slowed the reaction.
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The only thing that a catalyst does is to lower the activation energy, or energy needed to form the activated complex, the transition state found at the very top of the hill on your potential energy curve. Since not so much energy has to be supplied to start the reaction, it is not surprising that catalyzed reactions are usually faster than those that do not involve a catalyst