Collision theory, concentration and pressure Quiz
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5 questions, one answer each
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1. Which statement defines activation energy?
- A. The energy released in a reaction
- B. The minimum energy that colliding particles need for a reaction
- C. The average energy of the particles
- D. The energy needed to break all of the bonds
2. Why does increasing the concentration of a solution increase the rate?
- A. The particles move faster
- B. The activation energy is lower
- C. A greater proportion of collisions are successful
- D. There are more particles per unit volume, so more frequent collisions
3. What happens when the pressure of a gas mixture is increased at constant temperature?
- A. Collisions become more frequent because there are more particles per unit volume
- B. The activation energy decreases
- C. The particles move faster
- D. The proportion of particles with energy ≥ Ea increases
4. Why do most collisions not lead to a reaction?
- A. The particles are too large
- B. The particles are in the wrong state
- C. Most particles have less energy than the activation energy
- D. The collisions are too slow
5. A gas-phase reaction is at constant temperature and volume. Which change has no effect on the rate?
- A. Adding more of one reactant
- B. Adding an inert gas
- C. Doubling the amount of both reactants
- D. Compressing the gases