If the activation energy for a given compound is found to be 103 kJ/mol, with a frequency factor of 4.0×1013 s-1 what is the rate constant for this reaction at 398 K? A) 3.9 × 1010 s-1 B) 1.2 s-1 C) 2.5 × 107 s-1 D) 8.2 s-1 E) 1.7 × 1010 s-1

Calculate the value of the reaction rate constant if the initial concentrations of "A" is 0.05M and that of "B" is 0.08M, considering B of second order and the reaction rate is 1.6 X10-3 M/s. a) 9 s-1b) 4 s-1c) 2 s-1d) 5 s-1

3) Step 1) A B + C (Fast, equilibrium) Step 2) CD+E (slow) Write a rate law that is consistent with this mechanism. What is the overall reaction?

5. The reaction A →B+C is known to be first order in A. Below are data showing the concentration of A as a function of reaction time. Time, min [A], M 5.00 x 10-2 4.30 x 10-2 5 10 3.70 x 10-2 2.74 x 10-2 1.51 x 10-2 20 40 1.12 x 10-2 8.26 x 10-3 50 60 (a) What is the average rate of reaction between 5 and 20 min? Report the units as well as the numbers. (b) Plot the data above, showing the concentration of A as a function of the time. From your graph, determine the instantaneous rate of reaction at 40 min. Report the units as well as the numbers. (c) Plot In [A] versus time. Estimate the rate constant for this first-order reaction from your graph. Report the units as well as the numbers.