The rate constant for the decomposition of hydrocarbons is 2.418 x 10^-5 s^–1at 546 K. If the energy of activation is 179.9 kJ/mol, what will be the value of pre-exponental factor.

Solution

According to the Arrhenius equation

K = 2.418 \times 10^{- 5} S^{- 1} Ea = 179.9 kJ / mol . K = Ae - Ea / RT \log K = \log A - \frac{Ea}{2.303 R} logA = \log 0.0000241 + \frac{179.9}{2.303 \times 8.314 \times 546} logA = \log 0.0000241 + 0.02 A = 3.9 \times 16^{2} s^{- 1} .

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