Question #2 The kinetics of the gas-phase reaction between nitrogen dioxide, NOz

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Question #2 The kinetics of the gas-phase reaction between nitrogen dioxide, NOz (A) and trichloroethene (B) have been investigated over the range 303-362 2 K. The reaction extent, with the reaction carried out ina constant-volume batch reactor, was determined from measurements of infrared absorption intensities, which were converted into corresponding pressures by calibration. The products of the reaction are nitrosyl chloride NOCI, (R), and glyoxyloxyl chloride(S) In a series of seven experiments at 323.1 K, the initial pressures, PAo and PBo Were varied, and the partial pressure of NOC, PRwas measured after a certain length of time. Results are as follows t/min182.2360.4 360.8 435.3 332.8 PAo/kPa 3.97 Peo/kPa 7.16 120 2.49 8.57 0.027 182.1 2.08 9.26 0.04 5.55 7.66 PR/kPa 0.053 0.147 0.107 0.067 3.99 6.89 2.13 6.77 3.97 3.03 0.04 a. Write the chemical equation representing the stoichiometry of the reaction b. Can the course of the reaction be followed by measuring (total) pressure rather than by the method described above? Explain. c. Determine the form of the rate law and the value of the rate constant (in units of L mol s)at 323.1 K. with respect to NO2 (A). Derive all necessary equations

Explanation / Answer

a. 2NO2 + C2HCl3 ----> 2NOCl + C2HClO2

b. no, I don't think determining the total pressure would be much helpful. measuing the partial pressure of the product gives you and idea of the extent of reaction completion.

c. the valus of no2 are so variating that I cannot determine the order of reaction

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