Explain how a catalyst may increase the rate of chemical reaction?
A catalyst lowers the acitvation energy of a reaction.
A catalyst lowers the activation energy of a reaction without affecting the reaction in any way.
Lowers the activation energy of the reaction. Like a hill, it makes the hill lower so the reaction can proceed faster and at lower temps. Delta G is lowered. Meaning less energy is needed to move the reaction forward. Catalysts (enzymes) are substrate specific. only specified compounds like a right glove only fits a right hand and not the left hand.
A catalyst speeds up the reaction by lowering the energy needed for a reaction to occur.
Catalysts lower the activation energy (that is, the energy needed for a reaction to proceed) in either the final product or the intermediates. It can do this in a number of ways, including conformational (shape) changes in the intermediates (such as in complex organic molecules), changing the intermediates that form (alternate reaction pathway) or by changing the reactant in a certain way (like sulfuric acid stripping a proton off of a molecule so that nitric acid can bind to it and nitrate it, which would otherwise be energetically unfavorable). In English, catalysts change the molecules so it doesn't take as much energy for the reaction to take place. Think of jumping a hurdle: the same height on either side of it (reactant and product), but if you lower the hurdle (reduce the activation energy) it's easier to get to the other side.
