Kinetics Problem Set 1 Answer the following questions on a separate sheet of paper. The questions must be done in the order given. If you are skipping a question, leave space in case you decide to return to the problem. You do not need to recopy the question, simply indicate its number in the upper left corner. Do not type your answers. In most cases when the submission is typed blackboard will change the formatting on your submission. Write your answers with blue or black ink.

1. Show how the rate of disappearance of PCl3 relates to the rate of disappearance of NH3 and the rate of appearance of HCl and P(NH2)3? PCl3(g) + 3NH3(g) 3HCl(g) + P(NH2)3(g)

2. Using the following experimental data, determine the rate law and rate constant for the reaction. Experiment [H2] (M) [Cl2] (M) Initial Rate (M/s) 1 2.0 x 10-3 3.0 x 10-3 4.0 x 10-4 2 6.0 x 10-3 3.0 x 10-3 3.6 x 10-3 3 6.0 x 10-3 6.0 x 10-3 7.2 x 10-3

3. The second order reaction 2 CH4 C2H2 + 3H2 has a rate constant of 5.76 M-1min-1 at 1600 K. How long, in seconds, will it take for the concentration of CH4 to reduce from 1.25 M to 5.25 x 10-4M?

4. Answer the following questions based on the following rate law : rate = k[A]2 [B]3 .

a. By what factor will the rate of reaction change if the concentration of B is quadrupled.

b. By what factor will the rate of reaction change if concentration of A is increased 9 fold.

5. This reaction is first order with respect to CS2 with k = 2.8 x 10-7 s -1 at 1000. CS2 CS+S

a. If the initial CS2 concentration is 2.8 M, what is the CS2 concentration 28 days later?

b. How many hours must pass before a 15.0 g sample of CS2 decomposes so that only 2.00 g of CS2 remains?

c. What is the half life of CS2 at 1000 in seconds?

6. This reaction is second order with k = 0.0442 M-1 s -1 . 2C2F4 C4F8

a. The initial C2F4 concentration is 0.0675 M, what is the concentration of C2F4 1.5 minutes after the reaction begins?

b. What is the half-life of this reaction at these conditions in seconds?

7. Find activation energy (kJ/mol) for a reaction where the rate constant quadruples as the temperature increases from 298 K to 325 K.

8. The balanced equation for the reaction of the gases nitrogen dioxide and fluorine is: 2NO2(g) + F2(g) 2NO2F(g) A chemist suggested the following mechanism: Step # Equation Rate 1 NO2(g) + F2(g) NO2F(g) + F(g) Fast 2 F(g) + NO2(g) NO2F Slow

A. Determine the rate law based on the mechanism proposed. (Be sure to show all steps and logic)

B. In your opinion do you think this mechanism is likely to be correct? There is no right or wrong answer for this question as it is an opinion. However, you must support your answer using the determined rate law and your new knowledge about Kinetics.