The ozonization of pentene in carbon tetrachloride solution at 25 °C C3H10 + O3C3H1003 is first order in C3H10 and first order in 03. Complete the rate law for this reaction in the box below. Use the form k[A]"[B]".. , where '1' is understood for m, n .. (don't enter 1) and concentrations taken to the zero power do not appear. Rate = k[C3H1,][O,] In an experiment to determine the rate law, the rate constant was determined to be 1.24x105 M's1. Using this value for the rate constant, the rate of the reaction when [C3H10] = 3.41×10² M and [O3] = 2.52x10-2 M would be 9.16x10^4 Ms-!.

The ozonization of pentene in carbon tetrachloride solution at 25 °C C3H10 + O3C3H1003 is first order in C3H10 and first order in 03. Complete the rate law for this reaction in the box below. Use the form k[A]"[B]".. , where '1' is understood for m, n .. (don't enter 1) and concentrations taken to the zero power do not appear. Rate = k[C3H1,][O,] In an experiment to determine the rate law, the rate constant was determined to be 1.24x105 M's1. Using this value for the rate constant, the rate of the reaction when [C3H10] = 3.41×10² M and [O3] = 2.52x10-2 M would be 9.16x10^4 Ms-!.

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 ozonization of pentene in carbon tetrachloride solution at 25 °C C3H10 + O3C3H10O3 is first order in C3H10 and first order in O3. Complete the rate law for this reaction in the box below. Use the form k[A]"B"... , where '1' is understood for m, n. (don't enter 1) and concentrations taken to the zero power do not appear. Rate = In an experiment to determine the rate law, the rate of the reaction was determined to be 250 Ms-1 when [C3H10] = 9.52×10-2 M and [O3] = 2.41×10-² M. From this experiment, the rate constant is
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D Other Bookmarks [References) Use the References to access important values if needed for this question. The reaction of nitrogen dioxide with fluorine 2 NO2 + F22 NO2F is first order in NO2 and first order in F2. Complete the rate law for this reaction in the box below. Use the form k[A]m[B]"..., where '1' is understood for m, n ... (don't enter 1) and concentrations taken to the zero power do not appear. Rate = In an experiment to determine the rate law, the rate constant was determined to be 1.51x10-4 M-15-1 Using this value for the rate constant, the rate of the reaction when [NO2) = 1.95 M and [F2] = 2.97 M would be Ms-1, Submit Answer Try Another Wersion 2 item attempts remaining 7:15 PM 5/5/2022 SONY WEB K DISPLAY OFF One Touch Web Access Without Booting Up Delete F6 Num Lk Ser Lk Prt Sc Sys Ra Insert Pause F4 F7 BIG F12 F5 F8 F9 F10 F11 Break 1& Backspace - Home 6.
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