How do catalyst's increase the rate of a chemical reaction?

Answer 1

catalysts essentially reduce the energy it takes to make a chemical reaction go (meaning they lower the activation energy, if you're familiar with that).

catalysts are not consumed in the chemical reaction, so they can do this over and over again. also note: the effectiveness of catalysts (can) depend on temperature and concentration/amount

Answer 2

Essentially, catalysts speed up chemical reactions by reducing the amount of energy required for the reaction to occur. Catalysts are not consumed in the process, and so can do this many times. Some other factors that can affect a catalysts' ability to speed a process are temperature, concentration (of either the catalyst or the chemicals being reacted) and pH level. :) Good Luck

Answer 3

Catalysts are basically what starts the reaction. You need a catalyst to even get a reaction. Like a match for example. If you were trying to light \a candle, you couldn't just light the candle without some source of fire to start it. That source of fire would be your catalyst. A match works great for that obviously.

Answer 4

Catalysts work by providing an alternative pathway with lower activation energy for the reaction to occur. This lowers the barrier for the reactants to convert into products, thus increasing the rate of the chemical reaction without being consumed in the process.

Answer 5

They decrease the activation energy of that reaction.

Answer 6

Catalysts lower the activation energy required for a reaction or makes it easier to react. With more molecules possessing the requirement to react, the rate of reaction increases.

Answer 7

they reduce the amount of energy required by the reactants to activate the chemical reaction without involving in it themselves

Answer 8

We are unsure what you are asking. Please be more specific with your question to get an answer. Thanks.

Answer 9

particles collide