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 825.0 K? 𝑘=

Question

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 825.0 K?

𝑘=

Answer 1

Arrhenius equation: ln (k2/k1) = -Ea/R (1/T2 - 1/T1)

k1 = 6.1x10^-8s^-1

k2 = ?

Ea = 262 kJ/mol

R = 8.314 J/Kmol = 0.008314 kJ/Kmol

T1 = 600 K

T2 = 825K

ln (k2/6.1x10^-8) = - 262/0.008314 (1/825 - 1/600)

ln (k2/6.1x10^-8) = -31,513 (0.001212 - 0.001667)

ln (k2/6.1x10^-8) = -31,513 (-0.000455)

ln (k2/6.1x10^-8) = 14.34

(k2/6.1x10^-8) = 1689596

k2 = 0.103

(be sure to check the math)