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Question

From the following data answer the questions:
Reaction: A+B P

[A]M[B]MInitial rateM sec1
300 K400 K
2.5×1043.0×1055.0×1042.0×103
5.0×1046.0×1054.0×103
1.0×1036.0×1051.6×102
The energy of activation for reaction (kJ/mol) is:

A
20.83
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B
13.83
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C
15.23
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D
10.23
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Solution

The correct option is B 13.83
The arrhenius equation is k=A.eEa/RT.
At two different tempratures, this equation becomes lnk2k1=EaR[1T11T2]
Substitute values in the above equation.

ln2.0×1035.0×104

=EaR[13001400]

Ea=13.83 kJ/mol

Thus the energy of activation is 13.83 kJ/mol

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