The reaction
C4H8(g)⟶2C2H4(g)
has an activation energy of 262 kJ/mol. At 600.0 K, the rate constant, 𝑘, is 6.1×10−8 s−1. What is the value of the rate constant at 810.0 K?
helppppp please?
2020-10-13 11:06 am
回答 (1)
2020-10-13 11:21 am
✔ 最佳答案
Activation energy, Eₐ = 262 kJ mol⁻¹Gas constant, R = 0.008314 kJ mol⁻¹ K⁻¹
At T₁ = 600.0 K, k₁ = 6.1 × 10⁻⁸ s⁻¹
At T₂ = 810.0 K, k₂ = ? s⁻¹
Arrhenius equation:
ln(k₁/k₂) = (Eₐ/R) [(1/T₂) - (1/T₁)]
ln[(6.1 × 10⁻⁸)/k₂] = (262/0.008314) [(1/810.0) - (1/600.0)]
(6.1 × 10⁻⁸)/k₂ = 1.22 × 10⁻⁶
k at 810.0 K, k₂ = 5.0 × 10⁻² s⁻¹
收錄日期: 2021-04-24 08:09:55
原文連結 [永久失效]:
https://hk.answers.yahoo.com/question/index?qid=20201013030621AANyj6l