### 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

Answered: Image /qna-images/answer/da5d1d7f-b6b1-4d86-bb5c-578390ecdafe.jpg

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...

See similar textbooks

Similar questions

The reaction between N2O5 and water$$N2O5(g)+H2O(g)2HNO3(g)is a source of nitric acid in the atmosphere. The reaction is first order in each reactant. Write the rate law for the reaction.
20
The balanced chemical equation and rate law for the reaction between NO(g) and H2(g) at a particular temperature are 2NO(g) + 2H₂(g) → N₂(g) + 2H₂O(g) Rate = k[NO] [H₂] What is the reaction order with respect to nitric oxide AND the overall order of the reaction? 2,3 2,4 4,3 1,4 0,2
Consider the following fictitious balanced chemical equation below. In the first 315.0 seconds of the reaction, the concentration of B falls from 0.1597 M to 0.0672 M. What is the average rate of this reaction? 7 A (g) + 4 B (g) → 5 C (g) + 6 D (g)
- 1 Under certain conditions the rate of this reaction is zero order in hydrogen iodide with a rate constant of 0.0020 M·s 2 HI (g) → H, (g) + I, (g) Suppose a 4.0 L flask is charged under these conditions with 150. mmol of hydrogen iodide. How much is left 5.0 s later? You may assume no other reaction is important. Be sure your answer has a unit symbol, if necessary, and round it to the correct number of significant digits.
Consider this reaction: 2SO3 (g) →2SO₂(g) + O₂(g) At a certain temperature it obeys this rate law. rate = (0.894 M¹-s¹) [S0₂] Suppose a vessel contains SO3 at a concentration of 0.390 M. Calculate the concentration of SO3 in the vessel 8.60 seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits. M Explanation Check 0 10 Q Search a Ⓒ2023 McGraw Hill LLC. All Rights Reserved. Terms of Use O Privacy Center
Consider this reaction: 2HI (g) → H, (g) +I, (g) At a certain temperature it obeys this rate law. rate =(0,465 s)[HI Suppose a vessel contains HI at a concentration of 0.540M. Calculate the concentration of HI in the vessel 2.80 seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits.
The data shows that the rate depends on the concentration of the reactants. How else can a chemist increase the rate of reaction?
- 1 Under certain conditions the rate of this reaction is zero order in ammonia with a rate constant of 0.0080 M's : 2 NH3 (g) → N, (g)+3 H, (g) Suppose a 5.0 L flask is charged under these conditions with 300. mmol of ammonia. How much is left 2.0 s later? You may assume no other reaction is important. Be sure your answer has a unit symbol, if necessary, and round it to 2 significant digits. x10 ?
- 1 Under certain conditions the rate of this reaction is zero order in hydrogen iodide with a rate constant of 0.0045 M's : 2 HI (g) → H, (g)+I, (g) Suppose a 250. mL flask is charged under these conditions with 350. mmol of hydrogen iodide. How much is left 80. s later? You may assume no other reaction is important. Be sure your answer has a unit symbol, if necessary, and round it to the correct number of significant digits. x10