The rate of the reaction NO2 (g) + CO (g) → NO (g) + CO2 (8) depends only on the concentration of nitrogen dioxide below 225°C. At a temperature below 225°C, the following data were collected: Time(s) [NO,J(mol/L) 0.500 1.20 x 10° | 0.444 3.00 x 103 0.381 | 4.50 × 10³ | 0.340 9.00 x 103 0.250 1.80 x 104 | 0.174 Determine the rate law, the integrated rate law, and the value of the rate constant. Calculate [NO,] at 2.70 x 104 s after the start of the reaction.

The rate of the reaction NO2 (g) + CO (g) → NO (g) + CO2 (8) depends only on the concentration of nitrogen dioxide below 225°C. At a temperature below 225°C, the following data were collected: Time(s) [NO,J(mol/L) 0.500 1.20 x 10° | 0.444 3.00 x 103 0.381 | 4.50 × 10³ | 0.340 9.00 x 103 0.250 1.80 x 104 | 0.174 Determine the rate law, the integrated rate law, and the value of the rate constant. Calculate [NO,] at 2.70 x 104 s after the start 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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NO2(g) + CO(g) NO(g) + CO2(g) The rate of the above reaction depends only on the concentration of nitrogen dioxide at temperatures below 225°C.At a temperature below 225°C the following data were obtained: Time(s) [NO2](mol/L) 0 0.440 1.55×103 0.418 3.88×103 0.389 5.81×103 0.368 1.16×104 0.317 2.32×104 0.248 Which of the following expressions for the rate law (either differential or integrated) are completely consistent with the above experimental data. ln([NO2]/[NO2]0) = -kt [NO2] = [NO2]0 - kt d[NO]/dt = k[NO2] k[NO2]2 = d[CO2]/dt 1/[NO2] - 1/[NO2]0 = kt Calculate the rate constant (k). Enter the numerical value and corresponding units.
Given the following reaction mechanism: What is the overall reaction? Identify the catalyst. Identify the intermediates.
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