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A reaction has a rate constant of 1.23 x 10 ^-2 /s at 400 K and .688/s...

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Chemistry

Areaction has a rate constant of 1.23 x 10 ^-2 /s at 400 K and.688/s at 450K.
What is the activation barrier for the reaction and what isthe value of the rate constant at 425 K ?

Answer & Explanation Solved by verified expert
3.6 Ratings (635 Votes)

logK2/K1   = Ea/2.303R * [1/T1 -1/T2]

log0.688/0.0123   = Ea/2.303*8.314 *[1/400 -1/450]

1.7476                 = Ea/19.1471* [0.0025 -0.0022]

1.7476               = Ea*0.0003/19.1471

Ea   = 1.7476*19.1471/0.0003 = 111538joules = 111.538Kj

logK2/K1   = Ea/2.303R * [1/T1 -1/T2]

log0.688/K2 = 111538/2.303*8.314 *[1/400 -1/425]

  log0.688/K2      = 111538/19.1471* [0.0025 -0.0023]

                           = 5825*0.0002

                           = 1.165

0.688/K2            = 101.165

0.688/K2            = 14.621

K2 = 0.688/14.621 = 0.04705sec-1 >>>> answer
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