To use the Arrhenius equation to calculate the activation energy. As temperature rises, the average kinetic...

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To use the Arrhenius equation to calculate the activation energy. As temperature rises, the average kinetic...

To use the Arrhenius equation to calculate the activation energy.

As temperature rises, the average kinetic energy of molecules increases. In a chemical reaction, this means that a higher percentage of the molecules possess the required activation energy, and the reaction goes faster. This relationship is shown by the Arrhenius equation

k=Ae−Ea/RT

where k is the rate constant, A is the frequency factor, Ea is the activation energy, R = 8.3145 J/(K⋅mol) is the gas constant, and T is the Kelvin temperature. The following rearranged version of the equation is also useful:

ln(k2k1)=(EaR)(1T1−1T2)

where k1 is the rate constant at temperature T1, and k2 is the rate constant at temperature T2.

The rate constant of a chemical reaction increased from 0.100 s−1 to 3.20 s−1 upon raising the temperature from 25.0 ∘C to 35.0 ∘C .

What is the activation energy of the reaction?

Express your answer numerically in kilojoules per mole.

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Answer 1

Answer #1

en (K2/14) - tEa a 1 (250= 298 K7 am 0.100) - testo aby b) – 264 467.6J/mol or - 264047165 mol

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