Worksheet: Collision Theory

In this worksheet, we will practice using collision theory to describe the effect of solvent, temperature, and concentration on reaction rates.


Increasing the temperature usually causes the rate of a reaction to increase. Which of the following is not usually a cause of this effect?

  • AMore molecules exceed the activation energy for the reaction.
  • BMolecules collide more frequently.
  • CThe average kinetic energy of molecules is increased.
  • DChemical bonds vibrate more strongly.
  • EElectrons are promoted to higher-energy orbitals.


When a molecule of O2 collides with a molecule of CO, a molecule of CO2 may be formed. Which of the following is not a requirement for this reaction to take place?

  • AThe O2 molecule collides with the carbon atom of the CO molecule.
  • BValence electrons in the CO molecule are excited to a higher energy level before the collision takes place.
  • CThe molecules collide at an angle that allows for strong orbital overlap.
  • DThe kinetic energy of the colliding molecules exceeds the activation energy for the reaction.
  • EThe collision produces a transition state in which the original CO bond is lengthened.


Magnesium reacts with aqueous hydrochloric acid to form aqueous magnesium chloride. Which of the following quantities could be reduced to increase the rate of this reaction?

  • ATemperature
  • BAcid volume
  • CMagnesium surface area
  • DpH
  • EMagnesium mass

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