for a given reaction the value of the activation energy is 5.12 kJ/mol, given th

Question

for a given reaction the value of the activation energy is 5.12 kJ/mol, given that the rate constant at 25 degree Celsius is 1.55x10-3 I/s. what is the value of the rate constant at 45 degree Celsius ? for a given reaction the value of the activation energy is 5.12 kJ/mol, given that the rate constant at 25 degree Celsius is 1.55x10-3 I/s. what is the value of the rate constant at 45 degree Celsius ? for a given reaction the value of the activation energy is 5.12 kJ/mol, given that the rate constant at 25 degree Celsius is 1.55x10-3 I/s. what is the value of the rate constant at 45 degree Celsius ?

Explanation / Answer

we know that

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

given

k1 = 1.55 x 10-3

T1 = 25 C

T1 = 25 + 273

T1 = 298 K

Ea = 5.12 x 1000

T2 = 45 C = 318 K

so

using these values

we get

ln ( k2 / 1.55 x 10-3) = ( 5.12 x 1000 / 8.314) ( 1/298 - 1/318)

solving

we get

k2 = 1.765 x 10-3

so

the rate constant at 45 C is 1.765 x 10-3

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