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

A reaction 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 is the value of the rate constant at 425 K ?

Solutions

Expert Solution

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 = 10^1.165

0.688/K2 = 14.621

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

queen_honey_blossom answered 1 year ago

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