How do catalysts affect a chemical reaction?(1 point)
Responses
lose activation energy
lose activation energy
lower activation energy
lower activation energy
provide activation energy
provide activation energy
increase activation energy
lower activation energy
What happens during rusting of an iron nail?(1 point)
Responses
Iron and sulfur combine to form iron sulfide.
Iron and sulfur combine to form iron sulfide.
Sulfur and oxygen combine to form a sulfur dioxide coating.
Sulfur and oxygen combine to form a sulfur dioxide coating.
Iron and oxygen combine to form iron oxide.
Iron and oxygen combine to form iron oxide.
Sulfur, iron, and oxygen combine to form iron sulfoxide.
Iron and oxygen combine to form iron oxide.
What does the forward arrow in a chemical equation mean?(1 point)
Responses
The reaction proceeds slowly.
The reaction proceeds slowly.
The reaction yields something.
The reaction yields something.
The reaction proceeds quickly.
The reaction proceeds quickly.
The reaction is reversible.
The reaction yields something.
Which kind of reaction is photosynthesis?(1 point)
Responses
light-independent
light-independent
temperature-independent
temperature-independent
exothermic
exothermic
endothermic
endothermic
Photosynthesis requires which kind of energy?(1 point)
Responses
mechanical energy
mechanical energy
light energy
light energy
heat energy
heat energy
thermal energy
light energy
Catalysts do not increase the activation energy of a chemical reaction. Instead, they have the opposite effect by lowering the activation energy. The activation energy is the minimum amount of energy required for a reaction to take place.
To understand how catalysts lower the activation energy, you can think of a chemical reaction as a hill that reactant molecules need to overcome in order to reach the product state. The hill represents the energy barrier that the reactants must surpass for the reaction to occur.
Catalysts work by providing an alternative reaction pathway with a lower activation energy. They achieve this by forming temporary bonds with the reactant molecules, which alters the mechanism of the reaction. This new pathway has a lower energy barrier, making it easier for the reactants to reach the product state.
It is important to note that catalysts themselves are not consumed during the reaction and can be reused multiple times. They merely facilitate the reaction by lowering the activation energy, allowing it to happen more quickly and efficiently.