a) a certain first order reaction has a rate constant of2.95*10-1 s-1 at 24 degrees C. What is thethe value of k(rate constant) at 67 degreeC if Ea =87.0 kJ/mol? b) a certain first order reaction has a rate constant of2.95*10-2 s-1 at 24 degree C. What is thevalue of k(rate constant) at 67 degree C if Ea =123 kJ/mol? a) a certain first order reaction has a rate constant of2.95*10-1 s-1 at 24 degrees C. What is thethe value of k(rate constant) at 67 degreeC if Ea =87.0 kJ/mol? b) a certain first order reaction has a rate constant of2.95*10-2 s-1 at 24 degree C. What is thevalue of k(rate constant) at 67 degree C if Ea =123 kJ/mol?
Explanation / Answer
According to Arrhenies Equation , K = A e -Ea /RT log K = log A - (Ea / 2.303RT) For two cases log(K'/K) = ( Ea / 2.303R ) [(1/T) - ( 1/T')] = ( 87000J / 2.303* 8.314J/mol-K ) [(1/297) - ( 1/340) ] = 1.94 K'/K= 10^1.94 = 87.096 K' = 87.096 * K = 87.096 * 2.95*10^-1 s^-1 = 25.693 s^-1 Simillarly do the second one. log K = log A - (Ea / 2.303RT) For two cases log(K'/K) = ( Ea / 2.303R ) [(1/T) - ( 1/T')] = ( 87000J / 2.303* 8.314J/mol-K ) [(1/297) - ( 1/340) ] = 1.94 K'/K= 10^1.94 = 87.096 K' = 87.096 * K = 87.096 * 2.95*10^-1 s^-1 = 25.693 s^-1 Simillarly do the second one.