The tabulated data were collected for the second-order reaction: Cl(g) + H2(g) → HCl(g) + H(g). Use an Arrhenius plot to determine the activation barrier and frequency factor for the reaction. Temperature (K) and Rate Constant (L/mol # s) are as follows: 90 K, 0.00357; 100 K, 0.0773; 110 K, 0.956; 120 K, 7.781.

Verified step by step guidance

1. Convert the given temperatures from Kelvin to the reciprocal of temperature in Kelvin (1/T) for each data point.
2. Take the natural logarithm of the rate constant (k) for each temperature to obtain ln(k).
3. Plot ln(k) on the y-axis against 1/T on the x-axis to create the Arrhenius plot.
4. Determine the slope of the line from the Arrhenius plot, which is equal to -Ea/R, where Ea is the activation energy and R is the universal gas constant (8.314 J/mol K).
5. Calculate the activation energy (Ea) using the slope, and determine the frequency factor (A) by finding the y-intercept of the line, which is equal to ln(A).