Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
expand_more
expand_more
format_list_bulleted
Related questions
Question
![Chapter 15: Chemical Kinetics
54. The tabulated data show the concentration of N₂O5 versus time for this reaction:
N₂O5(g) → NO3(g) + NO₂(g)
F5
Time (s)
0
25
50
75
100
125
150
175
200
[N₂O5] (M)
1.000
0.822
0.677
0.557
0.458
0.377
0.310
0.255
0.210
Determine the order of the reaction and the value of the rate constant. Predict the
concentration of N₂O5 at 250 s.
口 ▶
4-80^@@@60760@@ - @@G|O@
MacBook Air
➤11](https://content.bartleby.com/qna-images/question/218ad4fc-c68a-4fcc-979f-dfd70997cb14/7a240c15-5721-48ae-a39d-7b083a61fb62/u45adkk_processed.jpeg)
Transcribed Image Text:Chapter 15: Chemical Kinetics
54. The tabulated data show the concentration of N₂O5 versus time for this reaction:
N₂O5(g) → NO3(g) + NO₂(g)
F5
Time (s)
0
25
50
75
100
125
150
175
200
[N₂O5] (M)
1.000
0.822
0.677
0.557
0.458
0.377
0.310
0.255
0.210
Determine the order of the reaction and the value of the rate constant. Predict the
concentration of N₂O5 at 250 s.
口 ▶
4-80^@@@60760@@ - @@G|O@
MacBook Air
➤11
Expert Solution
This question has been solved!
Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.
This is a popular solution
Trending nowThis is a popular solution!
Step by stepSolved in 5 steps with 5 images
Knowledge Booster
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
- In an experiment, a sample of NaClO3 was 90% decomposed in 40. min. The rate of this reaction doubles for every 10°C rise in temperature. Approximately how long (in min) would this decomposition have taken if the sample had been heated 20°C higher?arrow_forwardWrite the reaction rate expressions for the reaction below in terms of the disappearance of the reactants and the appearance of products. Give the expressions for the disappearance of the reactants first, in the order written in the chemical equation. Then write the expressions for the appearance of the products in the order written in the chemical equation. Write the expressions in order of appearance in the equation in the form. where + is either a plus OR a minus sign, not both, X is an integer, and A is a chemical species. Do not include the state of matter. 1 A[4] At 4NH3(g) + 502(g) → 4NO(g) + 6H2O(g) 1 ΔΙ The rate = 4 At Δι A[ At Al Atarrow_forwardSome measurements of the initial rate of a certain reaction are given in the table below. [№₂] [H₂] initial rate of reaction 1.73M 1.09 M 0.969 M/s 5.52M 1.09 M 9.87 M/s 1.73 M 0.117 M 0.104 M/s Use this information to write a rate law for this reaction, and calculate the value of the rate constant k. Round your value for the rate constant to 3 significant digits. Also be sure your answer has the correct unit symbol. rate = k k=0arrow_forward
- A substance decomposes with a rate constant of 9.05 × 10⁻⁴ s⁻¹. How long does it take for 25.5% of the substance to decompose?arrow_forwardA substance decomposes with a rate constant of 9.05 x 10-4 s¯¹. How long does it take for 15.0% of the substance to decompose?arrow_forwardChapter 13, Question 69 X Your answer is incorrect. Try again. Phosphine (PH3) decomposes into phosphorus and molecular hydrogen: 4PH3(g) - P4(9) + 6H2(g) Experiments show that this is a first-order reaction, with a rate constant of 1.73 x 102 s at 650°C. Which of the following statements are true? Select all that apply. V The overall reaction is elementary. O The data allow E, to be evaluated. M The rate constant will be smaller than 1.73 x 10 2 s at 500°C. V The reaction PH3 - PH, + H might be the first, rate-determining step in the mechanism of this reaction.arrow_forward
- The rate constant for the decomposition of N2O(g) is 1 × 10−3 M−1 sec−1. Assuming the initial concentration of N2O(g) is 0.2M, which of the following statements is true? The reaction is first order and the half life is 630 seconds The reaction is second order and the half life is 5 seconds The reaction is second order and the half life is 630 seconds The reaction is zeroth order and the half life is 9 seconds. The reaction is first order and the half life is 9 secondsarrow_forwardCalculate the rate constant, k, for a reaction at 60.0 °C that has an activation energy of 77.7 kJ/mol and a frequency factor of 6.59 x 101 s-1. k =arrow_forwardThe rate constant for the second-order reaction: 2NOBr(g)→2NO(g) + Br2(g) is 0.80/(M·s) at 10°C. Starting with a concentration of 0.86 M, calculate the concentration of NOBr after 59 s.arrow_forward
- Consider the decomposition of dinitrogen pentoxide: 2N2O5(g) → 4NO2(g) + O2(g) If the rate of change for the formation NO₂ is +4.50 × 105 mol L-¹ s -¹, determine the rate of change for the decomposition of dinitrogen pentoxide. O -1.13 x 105 mol L-¹5-1 O +1.13 x 105 mol L-¹5-1 O -4.50 x 10-5 mol L-¹5-1 O -2.25 x 105 mol L-¹5-1 O +2.25 x 10-5 mol L-¹ 5-1arrow_forwardSome measurements of the initial rate of a certain reaction are given in the table below. [N-] H2 initial rate of reaction 0.539M 0.871M 7.00 x 10°M/s 0.539M 0.282M 7.34 x 10*M/s olo 0.172M 0.871M 7.13 x 10*M/s Ar Use this information to write a rate law for this reaction, and calculate the value of the rate constant k. Round your value for the rate constant to 3 significant digits. Also be sure your answer has the correct unit symbol. rate = k x10 k =arrow_forwardThe reaction rate for the decomposition of N,O5 to form NO2 and O2 was studied as a function of temperature. The first order reaction rate constants were found to be: T (K) k(s*) 273 7.9 x 107 298 3.5 x 105 308 1.4 x 104 318 5.0 x 104 328 1.5 x 10 3 338 4.9 x 103 What is the E, for this reaction in kJ/mol? Use Excel to plot the pertinent data and use linear regression to calculate the slope of the line connecting your data. Round your answer to 2 decimal places.arrow_forward
arrow_back_ios
SEE MORE QUESTIONS
arrow_forward_ios
Recommended textbooks for you
- ChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage Learning
ChemistryChemistryISBN:9781259911156Author:Raymond Chang Dr., Jason Overby ProfessorPublisher:McGraw-Hill Education
Principles of Instrumental AnalysisChemistryISBN:9781305577213Author:Douglas A. Skoog, F. James Holler, Stanley R. CrouchPublisher:Cengage Learning 
Organic ChemistryChemistryISBN:9780078021558Author:Janice Gorzynski Smith Dr.Publisher:McGraw-Hill Education
Chemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage Learning
Elementary Principles of Chemical Processes, Bind...ChemistryISBN:9781118431221Author:Richard M. Felder, Ronald W. Rousseau, Lisa G. BullardPublisher:WILEY
Chemistry
Chemistry
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Cengage Learning
Chemistry
Chemistry
ISBN:9781259911156
Author:Raymond Chang Dr., Jason Overby Professor
Publisher:McGraw-Hill Education
Principles of Instrumental Analysis
Chemistry
ISBN:9781305577213
Author:Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:Cengage Learning
Organic Chemistry
Chemistry
ISBN:9780078021558
Author:Janice Gorzynski Smith Dr.
Publisher:McGraw-Hill Education
Chemistry: Principles and Reactions
Chemistry
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:Cengage Learning
Elementary Principles of Chemical Processes, Bind...
Chemistry
ISBN:9781118431221
Author:Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:WILEY