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Collision theory

Chemistry • Reaction Rates • Knowledge-Based • 4 questions

Collision theory Knowledge-Based Download PDF

Chemistry · Chemical Kinetics · Chemistry · Reaction Rates

4 Chemistry practice questions on Collision theory. Questions that assess core concepts and understanding.

Questions

  1. 1.

    According to collision theory, which of the following changes increases the reaction rate by directly increasing the collision frequency per unit volume without altering the fraction of collisions that possess the activation energy?

    • A) Introducing a suitable catalyst into the reaction vessel
    • B) Raising the temperature of the reaction system
    • C) Decreasing the activation energy of the reaction pathway
    • D) Increasing the concentration of the reactant molecules
  2. 2.

    In collision theory, what does the steric factor (pp) in the reaction rate expression represent?

    • A) The fraction of collisions in which the reactant molecules are aligned with the correct spatial orientation to form products.
    • B) The fraction of colliding particles that possess kinetic energy equal to or greater than the activation energy.
    • C) The total number of collisions occurring between reacting molecules per unit volume per unit time.
    • D) The net reduction in the energy barrier achieved when an effective collision takes place.
  3. 3.

    According to collision theory, what is the primary reason that an increase in temperature causes a marked increase in reaction rate?

    • A) The fraction of colliding particles with kinetic energy exceeding the activation energy increases substantially.
    • B) The activation energy barrier for the reaction is lowered significantly.
    • C) The spatial orientation requirement of the colliding particles becomes less strict.
    • D) The net enthalpy change between reactants and products increases.
  4. 4.

    According to collision theory, which of the following conditions must be satisfied simultaneously for a collision between reactant molecules to result in a chemical reaction?

    • A) The molecules must collide with kinetic energy below the activation energy and in an arbitrary orientation.
    • B) The molecules must collide with kinetic energy at least equal to the activation energy and with a favorable molecular orientation.
    • C) The molecules must collide at maximum velocity regardless of their spatial orientation or activation energy threshold.
    • D) The molecules must collide with identical individual speeds while maintaining a strictly perpendicular angle of impact.