BRAINCAKEExam Style Question - 2
Question: A student added magnesium ribbon to 1.0 mol dm-3 hydrochloric acid, then repeated the experiment with 2.0 mol dm-3 acid, keeping everything else the same. Use collision theory to explain why the reaction is faster with the more concentrated acid, and why the rate of each reaction decreases as it proceeds. (4 marks)
In 2.0 mol dm-3 acid there are more H+ ions in the same volume, so there are more collisions per unit time between H+ ions and the magnesium surface.
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More in Kinetics
- Maxwell-Boltzmann Distribution
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- The Effect of Temperature on Reaction Rate
- Catalysts
- Catalytic Converters
- Exam Style Question - 1
- Exam Style Question - 3
- Exam Style Question - 4
All 14 lessons in Kinetics · All AQA AS-level Chemistry topics