Consider the tabulated rate data for the reaction below: [NO2], M | [F2], m Initial Rate, M/s 0.100 Еxp 1 Exp 2 Exp 3 Еxp 4 0.100 0.026 2 ΝO, (g) + F (g) +2NOF(g) 0.200 0.100 0.051 0.200 0.200 0.103 0.400 0.400 0.411 (a) Use the data to determine the rate law of the reaction.

Consider the tabulated rate data for the reaction below: [NO2], M | [F2], m Initial Rate, M/s 0.100 Еxp 1 Exp 2 Exp 3 Еxp 4 0.100 0.026 2 ΝO, (g) + F (g) +2NOF(g) 0.200 0.100 0.051 0.200 0.200 0.103 0.400 0.400 0.411 (a) Use the data to determine the rate law of the reaction.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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The following initial rate data are for the reaction of ICI with hydrogen: 2 ICI + H2- →I2 + 2 HCI Experiment [ICI],, M [H2]o, M Initial Rate, M s-1 1 0.339 7.80x10-2 |3.63х10-3 0.678 7.80x10-2 7.26x10-3 3 0.339 0.156 1.45x10-2 14 0.678 0.156 2.90x10-2 Complete the rate law for this reaction in the box below. Use the form k[A]m[B]" , 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-2s-1.
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10. The data below are for the reaction: 2 NO₂ (g) + F₂ (g) → 2 NO₂F (g) [NO₂] (M) 0.100 0.200 0.200 0.400 0.200 [F₂] (M) 0.100 0.100 0.200 0.400 0.400 Initial rate (M/s) 0.026 0.051 0.103 0.411 see part c a. Write the rate law for this reaction. b. Determine the rate constant for this reaction. Pay attention to units. c. Predict the initial rate of the reaction when [NO₂] = 0.200 M and [F₂] = 0.400 M. d. The mechanism of the reaction is suggested as two steps: NO₂+ F2 → NO₂F + F (fast) NO₂+ F→→ NO₂F (slow) Is your rate law consistent with this mechanism? Explain your answer, making any changes necessary to create consistency.
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