### Reaction Rate DeterminationThe rate of the reaction:\[ \text{NO}_2(g) + \text{CO}(g) \rightarrow \text{NO}(g) + \text{CO}_2(g) \]was determined in three experiments at 225°C. The results are provided in the following table:| Experiment | [NO$_2$]$_0$ (M) | [CO]$_0$ (M) | Initial Rate - Δ[NO$_2$]/Δt (M/s) ||------------|----------------------|---------------|-------------------------------------|| 1 | 0.263 | 0.826 | 1.44×10⁻⁵ || 2 | 0.263 | 0.413 | 1.44×10⁻⁵ || 3 | 0.526 | 0.413 | 5.76×10⁻⁵ |### Questions and Calculations#### Part 1*Instructions: Do not include spaces or multiplication signs in your answer.***Determine the rate law for this reaction. Do not include states of matter or spaces in your answer.**```plaintextRate law = [ ]```#### Part 2**Calculate the value of the rate constant at 225°C.**\[ k = \_\_\_\_\_\ \text{M}^{-1}\text{s}^{-1} \]#### Part 3**Calculate the rate of appearance of CO$_2$ when [NO$_2$] = [CO] = 0.550 M.**\[ \text{Rate} = \_\_\_\_\_\_\ \times 10^\_\_\_\ \text{M/s} \]### Analysis and ExplanationWhen determining the rate law and the rate constant, consider the following:- Compare experiments where the concentration of one reactant remains constant to observe the effect of changing the other reactant's concentration on the rate.- Use the method of initial rates to determine the order of the reaction with respect to each reactant.- Calculate the rate constant using the rate law and the data from any of the experiments.This exercise involves understanding concepts such as reaction orders, the method of initial rates, and the calculation of rate constants, which are fundamental to the study of

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The rate of the reaction NO₂(g) + CO(g) was determined in three experiments at 225°C. The results are given in the following table: 5th attempt Part 1 Rate law NO(g) + CO₂(g) Part 2 Do not include spaces or multiplication signs in your answer. Determine the rate law for this reaction. Do not include states of matter or spaces in your answer. X X₁ +. log cos. ő Experiment [NO2]o (M) [CO]o (M) Initial Rate -A[NO2]/At (M/s) 0.263 0.826 1.44x10-5 0.263 0.413 1.44x10-5 0.526 0.413 5.76x10-5 Part 3 1 2 3 Calculate the value of the rate constant at 225°C. M¹s¹ Calculate the rate of appearance of CO₂ when [NO₂] = [CO] = 0.550 M. x 10 M/s - See Periodic Table See H

The rate of the reaction NO₂(g) + CO(g) was determined in three experiments at 225°C. The results are given in the following table: 5th attempt Part 1 Rate law NO(g) + CO₂(g) Part 2 Do not include spaces or multiplication signs in your answer. Determine the rate law for this reaction. Do not include states of matter or spaces in your answer. X X₁ +. log cos. ő Experiment [NO2]o (M) [CO]o (M) Initial Rate -A[NO2]/At (M/s) 0.263 0.826 1.44x10-5 0.263 0.413 1.44x10-5 0.526 0.413 5.76x10-5 Part 3 1 2 3 Calculate the value of the rate constant at 225°C. M¹s¹ Calculate the rate of appearance of CO₂ when [NO₂] = [CO] = 0.550 M. x 10 M/s - See Periodic Table See H

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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