How do catalysts affect a chemical reaction?(1 point)
Responses
provide activation energy
provide activation energy
increase activation energy
increase activation energy
lose activation energy
lose activation energy
lower activation energy
lower activation energy
What happens during rusting of an iron nail?(1 point)
Responses
Iron and oxygen combine to form iron oxide.
Iron and oxygen combine to form iron oxide.
Sulfur and oxygen combine to form a sulfur dioxide coating.
Sulfur and oxygen combine to form a sulfur dioxide coating.
Sulfur, iron, and oxygen combine to form iron sulfoxide.
Sulfur, iron, and oxygen combine to form iron sulfoxide.
Iron and sulfur combine to form iron sulfide.
Catalysts lower activation energy.
Catalysts affect a chemical reaction by lowering the activation energy required for the reaction to occur. Activation energy refers to the minimum amount of energy that needs to be supplied to the reactant molecules for the reaction to take place.
By providing an alternate pathway for the reaction to occur, catalysts can lower the activation energy. This is done by interacting with the reactant molecules, stabilizing them in a way that makes it easier for the reaction to proceed. Catalysts themselves are not consumed in the reaction and can be used repeatedly.
To understand how catalysts lower activation energy, you can consider the reaction energy diagram. It represents the energy changes that occur during a chemical reaction. Without a catalyst, the reactants need to overcome a high energy barrier (activation energy) before they can convert to products. However, with a catalyst, this energy barrier is reduced, allowing the reaction to happen more easily and at a faster rate.
In summary, catalysts lower the activation energy by providing an alternative reaction pathway, thus accelerating the rate of the chemical reaction.