We can use the following formula
ln(k2/k1) = Ea/R x (1/T1 - 1/T2)
Ea is the activation
energy of the reaction in J/mol = 66000 J/mol
R is the ideal gas constant = 8.3145 J/K·mol
T1 and T2 are temperatures in
Kelvin
T1 = 273 K And T2 = 273 + 74 = 347
K
k1 and k2 are rate constants of reaction at
T1 and T2
K1 = 2.4 x 10-5 K2 = ?
ln (K2 / 2.4 x 10-5) = 66000 J/mol / 8.3145 J/K·mol [1/273 - 1/347]
ln K2 - ln 2.4 x 10-5 = 6.2
ln K2 = -4.4396
Log K2 = 1.9277
K2 = 1.18 x 10-2 M-1 s-1
Hence rate constant of the reaction at 740C is 1.18 x 10-2 M-1 s-1
= Objective Knowledge Check Question 6 The rate constant of a certain reaction is known to...
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