Part A A certain reaction has an activation energy of 67.0 kJ/mol and a frequenc

Question

Part A

A certain reaction has an activation energy of 67.0 kJ/mol and a frequency factor of A1 = 4.70×1012 M1s1 . What is the rate constant, k, of this reaction at 29.0 C ? Express your answer with the appropriate units. Indicate the multiplication of units explicitly either with a multiplication dot (asterisk) or a dash.

Part B

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

Part A : Using Arrhenius equation,

rate constant k,

k = Ae^(-Ea/RT)

with,

A = 4.70 x 10^12 M-1/s-1

Ea = 67 kJ/mol

R = gas constant

T = 29 + 273 = 302 K

we get,

rate constant (k) = 4.70 x 10^12 x e^(-67000/(8.314 x 302)) = 12.111 M-1.s-1

Part B : ln(k2/k1) = Ea/R[1/T1 - 1/T2]

with data from above,

ln(185/109) = Ea/8.314[1/352 - 1/426]

Energy of activation (Ea) = 8.916 kJ/mol

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