When a collision occurs between two reactant particles that, between them, have the required minimum kinetic energy, or activation energy, a product does not always form. Which of the following reasons explains this?
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small surface area
Technically particles have to have the right orientation, sufficient kinetic energy, and all that good stuff. When you raise the temperature, the fraction of particles that have sufficient kinetic energy to and are in the proper orientation increases, so the probability goes up. So higher temperature is a must, over lower temperature.
When you increase concentration, that's more particles per a certain volume, that increases the number collisions between particles, and the likelihood your particles will collide to form your products. I believe surface area has the same effect.
Thoughts? @arindameducationusc @Rushwr@taramgrant0543664 I don't think that it's temperature. it's gotta be unfavorable geometry. (surface area and, low concentration) i think have a similar effect.