Learning Goal: To use the Arrhenius equation to calculate the activation energy.

Question

Learning Goal: 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: 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 3.00s_1 upon raising the temperature from 25.0 degree C to 49.0 degree C. Calculate the value of (1/T2 - 1/ T1) Express your answer numerically. Calculate the value of ln(k2/k1) Express your answer numerically. What is the activation energy of the reaction? Express your answer numerically in kilojoules pei mole.

Explanation / Answer

A)(1/T2 - 1/T1) =(1/322 - 1/298)= -2.5*10^-4.

(B) ln(K2/K1)=ln(3/0.1)

=ln30

=3.4012

(c) activation energy=188.4 kJ/mol

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