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Another first-order reaction also has a rate constant of 3.00×10−2 s−1 at 15 ∘C. What is...

Another first-order reaction also has a rate constant of 3.00×10−2 s−1 at 15 ∘C. What is the value of k at 67 ∘C if Ea = 131 kJ/mol ?

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Answer #1

The Arhenius equation is given by K= Koe (-Ea/RT)

Ea= activation energy and T = temperature in K

at two different temperatures T1 and T2, let the rate constants be K1 and K2. Arhenius equation can be written as

ln (K2/K1)= (Ea/R)*(1/T1-1/T2)

Ea=130 Kj/mol =130*1000 J/mol R= 8.314 j/mol.K T1= 15 deg.c =15+273.15= 288.15K and T2= 67+273.15K= 340.15K, K1= 3*10-2/s and K2=?

therefore

ln(K2/K1)= (131*1000/8.314)*(1/288.15-1/340.15)=8.4

K2/K1= exp(8.3)=4188.09

K2= 3*10-2*4188.09=125.6427/s

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