Why does increasing pressure increase the rate of reaction?

Why does increasing pressure increase the rate of reaction?

• A. Particles are squeezed closer together
• B. Temperature increases
• C. More exposed surface area
• D. Activation energy increases

Answer: (A)

Raising pressure increases rate of reaction because, for gases, the rate depends on how often reacting particles collide. When pressure goes up, gas molecules are squeezed closer together, effectively increasing their concentration. More molecules in the same volume means more collisions per second, so there are more opportunities for collisions that lead to reaction. Temperature and the activation energy aren’t changed by pressure, and changing pressure doesn’t increase surface area or alter the energy barrier itself; it simply makes collisions more frequent. So the best explanation is that particles are squeezed closer together, boosting collision frequency and speeding up the reaction.

Raising pressure increases rate of reaction because, for gases, the rate depends on how often reacting particles collide. When pressure goes up, gas molecules are squeezed closer together, effectively increasing their concentration. More molecules in the same volume means more collisions per second, so there are more opportunities for collisions that lead to reaction. Temperature and the activation energy aren’t changed by pressure, and changing pressure doesn’t increase surface area or alter the energy barrier itself; it simply makes collisions more frequent. So the best explanation is that particles are squeezed closer together, boosting collision frequency and speeding up the reaction.