Chemists commonly use a rule of thumb that an
increase of 10 K in temperature doubles the
rate of a reaction. What must the activation
energy be for this statement to be true for a
temperature increase from 25°C to 35°C?
Ea = 53 kJ
我完全看不懂，麻煩翻譯兼解答，謝謝
A Model for Chemical Kinetics
2010-06-16 10:48 pm
回答 (1)
2010-06-16 11:30 pm
✔ 最佳答案
化學家有一個經驗法則，就是溫度上升 10 K，反應速率就會變成兩倍。溫度由 25°C 上升至 35°C，若要使以上陳述正確，則反應的活化能必須是多少？ k1/k2 = 1/2
R = 8.314 J mol⁻¹ K⁻¹
T1 = 273 + 25 = 298 K
T2 = 273 + 35 = 308 K
Arrhenius equation:
ln(k1/k2) = -(Ea/R)[(1/T1) - (1/T2)]
ln(1/2) = -(Ea/8.314)[(1/298) - (1/308)]
Activation energy, Ea = 53000 J mol⁻¹ = 53 kJ mol ⁻¹
參考: 老爺子
收錄日期: 2021-05-01 01:04:03
原文連結 [永久失效]:
https://hk.answers.yahoo.com/question/index?qid=20100616000010KK04662