**The Reaction of Nitrogen Dioxide with Carbon Monoxide****Reaction:** \[ \text{NO}_2 + \text{CO} \rightarrow \text{NO} + \text{CO}_2 \]- The reaction is second order in \(\text{NO}_2\) and zero order in \(\text{CO}\).**Rate Law:** Complete the rate law for this reaction in the box below. Use the form \( k[\text{A}]^m[\text{B}]^n \ldots \), where '1' is understood for \( m, n \ldots \) (do not enter 1) and concentrations taken to the zero power do not appear.**Rate =** \[ k[\text{NO}_2]^2 \]**Experimental Determination:** In an experiment to determine the rate law, the rate constant was determined to be \( 0.780 \, \text{M}^{-1}\text{s}^{-1} \). Using this value for the rate constant, the rate of the reaction when \([\text{NO}_2] = 0.400 \, \text{M}\) and \([\text{CO}] = 0.372 \, \text{M}\) would be:**Rate =** \(k[\text{NO}_2]^2 = 0.780 \times (0.400)^2 = 0.1248 \, \text{Ms}^{-1}\).(Note: Since CO is zero order, its concentration does not affect the rate and does not appear in the rate law.) **The reaction for the formation of phosgene from carbon monoxide and chlorine**\[ \text{CO} + \text{Cl}_2 \longrightarrow \text{COCl}_2 \]is first order in CO and second order overall.**Complete the rate law for this reaction in the box below.**Use the form k[A]^m[B]^n..., where '1' is understood for m, n... *(don't enter 1)* and concentrations taken to the zero power do not appear.**Rate =** [Text box]

Problem # 1 It is given that the reaction is second order in NO2 and zero order in CO . Thus the…

The reaction of nitrogen dioxide with carbon monoxide NO, + CONO0 + CO2 is second order in NO, and zero order in CO. Complete the rate law for this reaction in the box below, Use the form k[A]™[B]"... , where 'l' 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 0.780 M's. Using this value for the rate constant, the rate of the reaction when [NO,] = 0.460 M and [CO] = 0.372 M would be Ms!.

The reaction of nitrogen dioxide with carbon monoxide NO, + CONO0 + CO2 is second order in NO, and zero order in CO. Complete the rate law for this reaction in the box below, Use the form k[A]™[B]"... , where 'l' 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 0.780 M's. Using this value for the rate constant, the rate of the reaction when [NO,] = 0.460 M and [CO] = 0.372 M would be 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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