生成物-时间
读数
发生了什么
分子只有在以足够的能量碰撞时才会反应。提高浓度让同样的空间里有更多分子，碰撞就更频繁。提高温度让每次碰撞更容易成功（更多分子越过活化能）。两者都会让生成物曲线更陡：开始时很快，随着反应物用完逐渐变平。
- Rate equationrate = k [A] [B]
- Arrhenius equationk ∝ e−Ea / RT
考试大纲
- GCSE Chemistry AQA 4.6.1, Edexcel, OCRrates of reaction and collision theory
- A-Level Chemistrythe Arrhenius equation and activation energy
挑战
先预测：这里哪种做法让反应更快：把 A 的量加倍，还是把温度升高 100 K？两种都试试，比较生成物曲线。
温度升高 100 K 的效果更大：速率常数随温度呈指数增长，而 A 的量加倍只会让碰撞频率加倍。
系统地学
GCSE Combined and Separate Science 中讲这个主题的课：先看分步讲解，再做考试风格的题目，每次数字都不同。 课程为英文。
常见问题
What is collision theory?
Particles react only when they collide with at least the activation energy and the right orientation. Anything that makes successful collisions more frequent speeds the reaction up.
Why does temperature speed up a reaction so much?
Particles move faster and collide more often, but the bigger effect is that far more collisions have enough energy to react. The rate constant grows exponentially, k ∝ e−Ea/RT.
How does a catalyst work?
It gives the reaction a different route with a lower activation energy, so more collisions succeed. It is not used up.
How do I find the activation energy from two rate constants?
Use ln(k₂/k₁) = (Eₐ/R)(1/T₁ − 1/T₂). If k doubles between 300 K and 310 K, Eₐ = 8.314 × ln 2 / (1/300 − 1/310) = 53.6 kJ/mol. That is the old rule of thumb that 10 K doubles the rate. Pick Activation energy under Solve for to see each step.