The activation energy for the gas phase isomerization of cyclopropane is 272 kj. (ch2)3ch3ch=ch2 the rate constant at 718 k is 2.30×10-5 /s. the rate constant will be /s at 753 k.

The answer is:

The rate constant K2 = 1.9 x 10^-4 1/s

The explanation:

According to Arrhenius equation:

ln(k₁/k₂) = Ea/R (1/T₂ - 1/T₁)

when K is the rate constant

and Ea is the activation energy

R is the ideal gas constant

T1 & T2 is a temperature at kelvin

when we have:

Ea = 272 KJ = 272000 J

R is the ideal gas constant 8.3145 J/Kmol

K1 = 2.3 x 10^-5 1/s    K2 = ?? that is we need to calculate

T1 = 718 K     T2 =753 K

So by substitution:

ln(k₁/k₂) = Ea/R (1/T₂ - 1/T₁)

㏑(2.3X10^-5/K2) = [272000/8.314](1/753-1/718)

∴ K2 = 1.9 x 10^-4 1/s

possibly, yes.

explanation:

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