The following initial rate data are for the reduction of nitric oxide with hydrogen: 2 NO + 2 H2 N2 + 2 H20 Experiment [NO]o, M [H2]o, M Initial Rate, M s-1 1 0.454 0.116 3.44x10-2 2 0.908 0.116 0.138 3 0.454 0.232 6.89x10-2 4 0.908 0,232 0.275 Complete the rate law for this reaction in the box below. Use the form k[A]m[B]n, where '1' is understood for m or n and concentrations taken to the zero power do not appear. Don't enter 1 for m or n. Rate = From these data, the rate constant is M-25-1.

The following initial rate data are for the reduction of nitric oxide with hydrogen: 2 NO + 2 H2 N2 + 2 H20 Experiment [NO]o, M [H2]o, M Initial Rate, M s-1 1 0.454 0.116 3.44x10-2 2 0.908 0.116 0.138 3 0.454 0.232 6.89x10-2 4 0.908 0,232 0.275 Complete the rate law for this reaction in the box below. Use the form k[A]m[B]n, where '1' is understood for m or n and concentrations taken to the zero power do not appear. Don't enter 1 for m or n. Rate = From these data, the rate constant is M-25-1.

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter11: Chemical Kinetics

Section: Chapter Questions

Problem 11.36PAE: The reaction NO(g) + O,(g) — NO,(g) + 0(g) plays a role in the formation of nitrogen dioxide in...

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The following rate constants were obtained in an experiment in which the decomposition of gaseous N2O; was studied as a function of temperature. The products were NO, and NO,. Temperature (K) 3.5 x 10_i 298 2.2 x 10"4 308 6.8 X IO-4 318 3.1 x 10 1 328 Determine Etfor this reaction in kj/mol.
Consider the following hypothetical data collected in two studies of the reaction 2A+2BC+2D Time(s) Experiment 1 [A] (mol/L) Experiment 2 [A] (mol/L) 0 1.0 102 1.0 102 10. 8.4 103 5.0 103 20. 7.1 103 2.5 103 30. ? 1.3 103 40. 5.0 103 6.3 104 In Experiment 1, [B]0 = 10.0 M. In Experiment 2, [B]0 = 20.0 M. Rate=[A]t a. Use the concentration versus time data to determine the rate law for the reaction. b. Solve for the value of the rate constant (k) for the reaction. Include units. c. Calculate the concentration of A in Experiment 1 at t =30.s
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For each of the following reaction diagrams, estimate the activation energy (Ea) of the reaction:
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