一題化學的問題~順便翻譯一下...

某反應的活化能是 54.0 kJ/mol。當溫度由 22℃ 上升至某較高溫度，其反應常數增加了的因數是 7.00 。計算較高的溫度。

Activation energy Ea = 54.0 kJ /mol = 54000 J /mol
Gas constant, R = 8.314 J /mol /K

At 22℃ :
Rate constant, k1 = k
Temperature, T1= 273 + 22 = 295 K

At the higher temperature :
Rate constant, k2 = k(1 + 7) = 8k
Temperature, T2 = ?

One form of Arrhenius equation :
ln(k1/k2) = -(Ea/R)[(1/T1) - (1/T2)]
(1/T1) - (1/T2) = -(R/Ea)ln(k1/k2)
1/T2 = (1/T1) + (R/Ea)ln(k1/k2)

Higher temperature, T2
= 1/[(1/T1) + (R/Ea)ln(k2k2)]
= 1/[(1/295) + (8.314/54000)ln(1/8)]
= 325.8 K
= 52.8℃

有些反應有54.0 KJ/mol活化能。 當溫度從22℃增加到一個更高的溫度，率常數由因素7.00增加。 計算更高的溫度。