The activation energy, Ea, for a particular reaction is 13.6 kJ/mol. If the rate constant at 754 °C is 24.5/min, at what temperature (in °C) will the rate constant be 14.9/min? (R = 8.314 J/mol • K)

Answer 1

Arrhenius equation

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

k1 = 24.5 min-1

k2 = 14.9 min-1

T1 = 754C + 273 = 1027 K

T2 = ?

Ea = 13.6 kJ/mol = 13,600 J/mol

R = 8.314 J/K-mol

ln (14.9/24.5) = -13,600/8.314 (1/T2 - 1/1027)

-0.4973 = -1636 (1/T2 - 0.0009737)

-0.4973 = -1636/T2 + 1.593

-2.09 = -1636/T2

T2 = 782K

T2 = 509ºC