How does a catalyst increase the rate of a chemical reaction?

Question

Does it decrease the average kinetic energy of the reactants of the reaction?
Does it increase the chance reactants will collide in the proper orientation?
Does it decrease the threshold energy value with which two particles must collide?

Or does it do something completely different?

Thank you in advance for your help!

Answer 1

doesnt it create the exact conditions where covalent bonde can be made or broken i do know it neither adds or takes away from the reaction

Answer 2

A more detailed answer is that the catalyst forms an activated complex (AC) with the reactants. This AC needs less energy to be formed compared to the AC that the reactants can form without the catalyst. The old bonds are broken, new bonds are formed and the new products split off from the catalyst. So the whole reaction needed less activation energy to take place and the catalyst did not get consumed.

Answer 3

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RE:
How does a catalyst increase the rate of a chemical reaction?
Does it decrease the average kinetic energy of the reactants of the reaction?
Does it increase the chance reactants will collide in the proper orientation?
Does it decrease the threshold energy value with which two particles must collide?

Or does it do something completely different?

Thank...

Answer 4

it depends on the type of the catalyst
all what you mentioned was correct, also the solid catalyst increase surface area available for reaction to occur

Answer 5

It lowers the activation energy needed for a reaction to occur

Answer 6

It lowers the activation energy necessary to start the reaction, thereby making it easier for the reaction to start and continue.

hope that helped a little.

Answer 7

it lowers the activation-energy barrier