Question

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: ln(k1k2)=(EaR)(1T2−1T1) 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 3.10 s−1 upon raising the temperature from 25.0 ∘C to 35.0 ∘C .

Part A

Calculate the value of (1T2−1T1) where T1 is the initial temperature and T2 is the final temperature.

Express your answer numerically.

Answer 1

Ln K_1/K_2 = Eq/R [1/T_2 - 1/T_1] K_1 = 0.100 s^-1 T_1 = 25.0 degree Celsius T_1 = 298 k T_2 = 35.0 degree Celsius T_2 = 308 K R = 8.314 [1/T_2 - 1/T_1] = (1/308 - 1/298) = 0.00325 - 0.00336 [1/T_2 - 1/T_1] = -0.00011