The rate constant at 325°C for the decomposition reaction C4H8 ⟶ 2 C2H4 is 6.1×10−8
s^−1, and the activation energy is 261 kJ per mole of C4H8. Determine the frequency factor for the reaction.

The Rate Constant At 325C For The Decomposition Reaction C4H8 2 C2H4 Is 6.1108s^1, And The Activation

Answers

Answer 1

The concept Arrhenius equation is used here to determine the frequency factor for the reaction. Here for the given reaction, the frequency factor is 3.814.

What is Arrhenius equation?

The Arrhenius equation explains the relationship between the activation energy and rate of the reaction. The lower the activation energy, higher will be the rate of reaction. The equation is:

[tex]k=A . e^{-E_{a} } / RT[/tex]

k - rate constant

A - frequency factor

Eₐ - activation energy

R - Gas constant

T - Temperature in Kelvin

261 kJ per mole = 261000 J/mol

325°C + 273 = 598 K

6.1 × 10⁻⁸ = A . e⁻261000/ 8.314 × 598

A = 3.814

Thus the frequency factor for the reaction is 3.814.

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