Initial rate constant is 0.0191 s-1 at initial 24°C,what is the rate constant at 120°C for a rxn w/ an activation energy of 43.4 kJ/mol?
Given that the initial rate constant is 0.0191 s-1 at an initial temperature of 24°C, what would the rate constant be at a temperature of 120°C for a reaction with an activation energy of 43.4 kJ/mol?
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ln(k2/k1)=(Ea/R) * (1/T1-1/T2)
Ea=43400 J/mol R=8.314 T1=297 T2=393 k1=0.0191
calculate k2 which would be 1.40/s