Part A Consider the following reaction: 2A + B ? C The initial rate is measured

Question

Part A

Consider the following reaction:

2A + B ? C

The initial rate is measured at several different reactant concentrations.

From the tabulated data, determine the rate law for the reaction in terms of reactant concentrations and k, the rate constant.

Rate=

The kinetics of the reaction between chlorine dioxide and ozone are relevant to the study of atmospheric ozone destruction. The value of the rate constant for the reaction between chlorine dioxide and ozone was measured at four temperatures. The results are as follows:

Calculate the value of the activation energy

1.27?1012

kJ/mol

Part B

Calculate the frequency factor for the reaction.

M-1 s-1

The kinetics of the reaction between chlorine dioxide and ozone are relevant to the study of atmospheric ozone destruction. The value of the rate constant for the reaction between chlorine dioxide and ozone was measured at four temperatures. The results are as follows:

Calculate the value of the activation energy

1.27?1012

kJ/mol

Part B

Calculate the frequency factor for the reaction.

M-1 s-1

I JUST NEED THE FREQUENCY FACTOR OF THE REACTION IN M-1*S-1 UNITS PLEASE

Explanation / Answer

As per the Arrhenius Equation:-

ln(k2/k1) = (Ea/R)*{(1/T1) - (1/T2) ; where k1 & k2 are the values of the rate constants at temperatures T1 & T2 respectively, R = Universal Gas Constant , Ea = energy of activation

Thus,

ln(62.8/34) = (Ea/8.314)*{(1/193) - (1/198)}

or, Ea = 38989.2 J = 38.989 kJ/mole

Also, as per Arrhenius Equation:-

lnk = lnA - (E/RT) ; where A = Frequency factor

Thus, ln38 = lnA - (38989.2/8.314*193)

or, lnA = 27.94

or, A = 1.36*!012

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