The reaction of N205 with gaseous H20 is a potentially important reaction in the chemistry of acid rain:N2O5(g) + H20(g) → 2HNO3(g)A chemist carried out kinetic studies on this reaction, obtaining the following data:Experiment A: [N,O5lo = 1.5 × 10-4M, [H2O]o = 0.025 M%3Dt (s)60120180240[N2O5] (105 M)6.115129.67.6Experiment B: [N2O5lo = 1.5 × 10-4M, [H2O]o = 0.050 M%3Dt (s)60120180240[N2O5] (10-5 M)159.66.13.92.5Use graphs to determine the rate law for this reaction, and evaluate the rate constant. In case of first ordertype "1".Rate =[N2O5] 1[H2O] ] 1k =iM-1s-1

The reaction of N205 with gaseous H20 is a potentially important reaction in the chemistry of acid rain: N2O5(3) + H2O(g) → 2HNO3(g) A chemist carried out kinetic studies on this reaction, obtaining the following data: Experiment A: [N2O5lo = 1.5 × 104 M, [H2O]o = 0.025 M t (s) 60 120 180 240 [N2O5] (10-5 M) 15 12 9.6 7.6 6.1 Experiment B: [N2O5lo = 1.5 × 104 M, [H2O]o = 0.050 M t (s) 60 120 180 240 [N2O5] (10-5 M) 3.9 15 9.6 6.1 2.5 Use graphs to determine the rate law for this reaction, and evaluate the rate constant. In case of first order type "1". Rate = [N2O5] 1 [H2O] 1 k k = i ! M-1 s-1

The reaction of N205 with gaseous H20 is a potentially important reaction in the chemistry of acid rain: N2O5(3) + H2O(g) → 2HNO3(g) A chemist carried out kinetic studies on this reaction, obtaining the following data: Experiment A: [N2O5lo = 1.5 × 104 M, [H2O]o = 0.025 M t (s) 60 120 180 240 [N2O5] (10-5 M) 15 12 9.6 7.6 6.1 Experiment B: [N2O5lo = 1.5 × 104 M, [H2O]o = 0.050 M t (s) 60 120 180 240 [N2O5] (10-5 M) 3.9 15 9.6 6.1 2.5 Use graphs to determine the rate law for this reaction, and evaluate the rate constant. In case of first order type "1". Rate = [N2O5] 1 [H2O] 1 k k = i ! M-1 s-1

Chemistry

9th Edition

ISBN:9781133611097

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

Chapter13: Chemical Equilibrium

Section: Chapter Questions

Problem 85AE: Suppose K = 4.5 103 at a certain temperature for the reaction PCl5(g)PCl3(g)+Cl2(g) If it is found...

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