A certain reaction has an activation energy of 69.0kJ/mol and a frequency factor

Question

A certain reaction has an activation energy of 69.0kJ/mol and a frequency factor of A1 = 6.60 Times 1012M-ls-1 What is the rate constant, k, of this reaction at 23.0 degree C ? Express your answer with the appropriate units. Indicate the multiplication of units explicitly either with a multiplication dot (asterisk) or a dash. The linear form of the Arrhenius equation The Arrhenius equation can be rearranged to a form that resembles the equation for a straight line: ln k = -(Ea/R) (1/T) + ln A y = m x + b where y is In k, m s the slope or -Ea/R, x is 1/T, and b is the y-intercept or ln A. The linearity of this equation is illustrated graphically in the image.(Figure 1) An unknown reaction was observed, and the following data were collected: Determine the activation energy for this reaction. Express your answer with the appropriate units.

Explanation / Answer

A) k = A * exp(-Ea/RT) => k = 6.6 * 10^12 * ex[(-69000/8.314*296) = 4.39

B) we have ln(k2/K1) = -Ea/R (1/T2-1/T1) => ln(426/352) = Ea/8.314 * (1/352-1/426)

solving you get Ea = 2438 J = 2.438 KJ

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