Worksheet: Collision Theory

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

Q1:

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.

Q2:

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.

Q3:

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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