Question

How does increasing the surface area of a reactant affect the rate of a reaction?

a) There are more frequent collisions with more surface area exposed.

b) Each collision is more energetic.

c) The fraction of collisions with the proper orientation increases with more surface area exposed.

d) The reaction pathway changes to one with a lower energy of activation when more surface area is exposed.

**The answer is A. I'm hoping for an explanation so I can fully understand the concept. What if I decreased the surface area? Any other scenarios? Thanks