Homework Help is Here – Start Your Trial Now!
Science
Chemistry
3 Kinetic Study: The lodine Clock Reaction Prelaboratory Questions Name Laboratory Section 1. Consider the following reaction: 2 N,O5 (g) 4 NO2 (g) + O2 (g) -> The initial concentration of N,O5 was 0.84 mol/L, and 35 minutes after initiating the reaction, all of the N,Os has been consumed. a) Calculate the average rate of the reaction over this 35-minute time interval. b) Is it correct to assume that the rate law is Rate = k[N,O5]² based on the balanced chemical equation? Briefly explain your answer. c) Suppose the reaction rate is determined by simultaneously measuring the rate of decrease of N,Os concentration (-ALN,O5]/At) and the rate of increase of NO, concentration (A[NO,]/At). Which rate will be higher and by what factor? (continued on next page) 137

3 Kinetic Study: The lodine Clock Reaction Prelaboratory Questions Name Laboratory Section 1. Consider the following reaction: 2 N,O5 (g) 4 NO2 (g) + O2 (g) -> The initial concentration of N,O5 was 0.84 mol/L, and 35 minutes after initiating the reaction, all of the N,Os has been consumed. a) Calculate the average rate of the reaction over this 35-minute time interval. b) Is it correct to assume that the rate law is Rate = k[N,O5]² based on the balanced chemical equation? Briefly explain your answer. c) Suppose the reaction rate is determined by simultaneously measuring the rate of decrease of N,Os concentration (-ALN,O5]/At) and the rate of increase of NO, concentration (A[NO,]/At). Which rate will be higher and by what factor? (continued on next page) 137

Chemistry
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
icon
Related questions
Question

1c

3 Kinetic Study: The lodine Clock Reaction Prelaboratory Questions Name Laboratory Section 1. Consider the following reaction: 2 N,O5 (g) 4 NO2 (g) + O2 (g) -> The initial concentration of N,O5 was 0.84 mol/L, and 35 minutes after initiating the reaction, all of the N,Os has been consumed. a) Calculate the average rate of the reaction over this 35-minute time interval. b) Is it correct to assume that the rate law is Rate = k[N,O5]² based on the balanced chemical equation? Briefly explain your answer. c) Suppose the reaction rate is determined by simultaneously measuring the rate of decrease of N,Os concentration (-ALN,O5]/At) and the rate of increase of NO, concentration (A[NO,]/At). Which rate will be higher and by what factor? (continued on next page) 137
Transcribed Image Text:3 Kinetic Study: The lodine Clock Reaction Prelaboratory Questions Name Laboratory Section 1. Consider the following reaction: 2 N,O5 (g) 4 NO2 (g) + O2 (g) -> The initial concentration of N,O5 was 0.84 mol/L, and 35 minutes after initiating the reaction, all of the N,Os has been consumed. a) Calculate the average rate of the reaction over this 35-minute time interval. b) Is it correct to assume that the rate law is Rate = k[N,O5]² based on the balanced chemical equation? Briefly explain your answer. c) Suppose the reaction rate is determined by simultaneously measuring the rate of decrease of N,Os concentration (-ALN,O5]/At) and the rate of increase of NO, concentration (A[NO,]/At). Which rate will be higher and by what factor? (continued on next page) 137
Expert Solution
trending now

Trending now

This is a popular solution!

steps

Step by step

Solved in 2 steps with 2 images

SEE SOLUTIONCheck out a sample Q&A here
Blurred answer
Knowledge Booster
Measurement
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.
Similar questions
  • SEE MORE QUESTIONS
Recommended textbooks for you
Chemistry
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
Principles of Instrumental Analysis
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
Organic Chemistry
Organic Chemistry
Chemistry
ISBN:
9780078021558
Author:
Janice Gorzynski Smith Dr.
Publisher:
McGraw-Hill Education
Chemistry: Principles and Reactions
Chemistry: Principles and Reactions
Chemistry
ISBN:
9781305079373
Author:
William L. Masterton, Cecile N. Hurley
Publisher:
Cengage Learning
Elementary Principles of Chemical Processes, Bind…
Elementary Principles of Chemical Processes, Bind…
Chemistry
ISBN:
9781118431221
Author:
Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:
WILEY
SEE MORE TEXTBOOKS