why does the catalyst decreases the activation energy of a chemical reaction?

Question

How does the catalyst decreases the activation energy of a chemical reaction

Answer 1

the catalyst helps the reaction proceed by allowing a separate path to reaction occur. nature uses enzymes to do this, humans use organic and inorganic chemicals

Answer 2

Increasing the temperature of the reaction would only increase the rate of the reaction by adding more energy to reach the activation energy, but it would have no effect whatsoever on the value of the activation energy. Increasing the concentrations of the reactants would shift your reaction equilibrium to the right, increasing your yield of products, and it may also increase the rate of the reaction; however, concentration of reactants would also have no effect on the "value" for energy of activation. Catalysts function to decrease the activation energy of a reaction by providing an alternative, lower energy path for the reaction. So, your answer should be (c) not (d)

Answer 3

The catalyst will actually help the reactants physically meet with each other and react. For example, platinum is often used as a catalyst in hydrogenation reactions because it grabs onto hydrogen atoms and passes them on to the reactant. In the end, the hydrogen atoms do not stick with the platinum or react with it, so platinum is purely a catalyst. It is in this manner that the activation energy is lowered.

Answer 4

The catalyst makes an easier pathway for the reaction, so it takes less activatiion energy.