Gaseous dinitrogen pentoxide, above its sublimation point of 47 oC, can decompose into nitrogen dioxide and molecular oxygen. The data below were measured at 60 oC in a closed container. t (sec) p(N2O5)(atm) Ln{p(N2O5)} 1/{p(N2O5)} 0.0 0.250 60.0 0.213 120.0 0.182 180.0 0.156 240.0 0.133 300.0 0.113

(a) (3 pts) Write the balanced decomposition reaction of dinitrogen pentoxide into nitrogen dioxide and oxygen using whole integer coefficients. (b) (8 pts) Does the reaction follow first-order or second-order kinetics? Use the data above by making two different plots to determine the proper rate law. Hint: begin by filling out the table and then graph the various columns verses time to determine the order of p(N2O5). (c) (2 pts) Determine the rate constant (include appropriate units) for this reaction at 60.0 oC. (d) (2 pts) What is the half-life (sec) for this reaction if the initial pressure of N2O5(g) would be 0.400 atm? (e) (2 pts) Write the complete rate law for this reaction. (f) (4 pts) What is the rate (M/sec) of dinitrogen pentoxide at t = 2.00 min? Hint: Use the Ideal Gas Law. (g) (4 pts) What is the rate (M/sec) of nitrogen dioxide formation at t = 2.00 min? Hint: Use relative rates. (h) (3 pts) One of several Lewis structures for dinitrogen pentoxide is shown above dinitrogen pentoxide is a planar molecule stabilized by resonance. Given this Lewis structure of N2O5(g) written above, write out a plausible three-step mechanism that agrees with the correct rate law for this reaction. Write the rate law for each elementary step in your mechanism and identify the rate-determining step. (i) (4 pts extra credit) If the activation energy for this decomposition is 103.5 kJ/mol, at what temperature (C) will the rate constant for this reaction be twice as large as at 60.0 C (see your answer to part (c) and assume that the frequency factor for this reaction remains constant as temperature varies).