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Use the data given in the above question to first determine the rate law before answering the second question (20) --> What is the value of the rate constant (k) with the appropriate units?

Use the data given in the above question to first determine the rate law before answering the second question (20) --> What is the value of the rate constant (k) with the appropriate units?

Chemistry
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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Use the data given in the above question to first determine the rate law before answering the second question (20) --> What is the value of the rate constant (k) with the appropriate units?

comoletely bublble in Determine the rate law for the production of nitrosyl fluoride (NO,F) that occurs according to the following balanced chemical equation: 2 NO: (g) + F2 (g) >2 NO,F (g) The following data were obtained from varying the concentrations of the reactants: Initial Rate (M/s) 2.16 x 10 4.30 x 104 2.61 x 104 5.22 x 104 [F] (M) [NO2] (M) 0.00130 Run 1 0.00479 Run 2 0.00259 0.00479 Run 3 0.00612 0.00123 Run 4 0.00612 0.00246 (A) (B) (C) (D) (E) Rate = k (NO2] [F] Rate = k (NO2]'(F2] Rate = k (NO2] Rate = k [NO2J²[F>105 Rate = k [NO2] [F:10.5 Using the data given for Question 19 (and the rate law that you derived), what is the value of the rate constant (k) with the appropriate units? (A) (B) (C) (D) (E) 34.7 s1 2.88 x 10? M's1 34.7 M's 6.23 x 106 s1 2.88 x 10s
Transcribed Image Text:comoletely bublble in Determine the rate law for the production of nitrosyl fluoride (NO,F) that occurs according to the following balanced chemical equation: 2 NO: (g) + F2 (g) >2 NO,F (g) The following data were obtained from varying the concentrations of the reactants: Initial Rate (M/s) 2.16 x 10 4.30 x 104 2.61 x 104 5.22 x 104 [F] (M) [NO2] (M) 0.00130 Run 1 0.00479 Run 2 0.00259 0.00479 Run 3 0.00612 0.00123 Run 4 0.00612 0.00246 (A) (B) (C) (D) (E) Rate = k (NO2] [F] Rate = k (NO2]'(F2] Rate = k (NO2] Rate = k [NO2J²[F>105 Rate = k [NO2] [F:10.5 Using the data given for Question 19 (and the rate law that you derived), what is the value of the rate constant (k) with the appropriate units? (A) (B) (C) (D) (E) 34.7 s1 2.88 x 10? M's1 34.7 M's 6.23 x 106 s1 2.88 x 10s
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