For a first order reaction, A → P, the temperature (T) dependent rate constant (k) was found to follow the equation: logk=2000T+6.0 the pre - exponential factor A and the activation energy Eα. respectively, are:
A
1.0×106s−1and9.2kJmol−1
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B
6.0s−1and16.6kJmol−1
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C
1.0×106s−1and16.6kJmol−1
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D
1.0×106s−1and38.3kJmol−1
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Solution
The correct option is D1.0×106s−1and38.3kJmol−1 The logarithmic form of Arrhenius equation is logk=logA−Eα2.303RT Given: logk=6−2000T Comparing the above two equations: logA=6⇒A=106 and Eα2.303R=2000 ⇒Eα=2000×2.303×8.314J =38.3kJmol−1