Ethyl chloride vapor decomposes by the first-order reaction c2h5cl → c2h4 hcl the activation energy is 249 kj/mol and the frequency factor is 1.6 * 1014 s-1. find the temperature at which the rate of the reaction would be twice as fast as when the reaction runs at 730.6 k. enter your answer numerically and in terms of kelvin.

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Chemistry

Omari

6 February, 02:34

Ethyl chloride vapor decomposes by the first-order reaction c2h5cl → c2h4 hcl the activation energy is 249 kj/mol and the frequency factor is 1.6 * 1014 s-1. find the temperature at which the rate of the reaction would be twice as fast as when the reaction runs at 730.6 k. enter your answer numerically and in terms of kelvin.

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Kyleigh Greene · Answer 1

Activation Energy Ea = 249 x 10^3 J/mol Frequency Factor = 1.6 Ă - 1014 sâ’1 Rate of reation is twice as fast with temperature change so k1/k2 = 1/2. Temperature T1 = 730.6, T2 = ? Gas constant R = 8.314 J / mole-K We have Arrhenius equation ln (k1 / k2) = (Ea / R) x [ (1/T1) - (1/T2) ] ln (1/2) = ((249 x 10^3) / 8.314) x [ (1/T2) - (1/730.6) ] ln (1/2) = 29.95 x 10^3 x [ (1/T2) - 0.0013687] - 0.69315 / (29.95 x 10^3) = (1/T2) - 0.0013687 (1/T2) - 0.0013687 = - 2.3 x 10^-5 1 / T2 = 0.0013455 T2 = 743.18 k