Homework Help is Here – Start Your Trial Now!
Science
Chemistry
The oxidation of nitrogen monoxide by oxygen at 25 °C 2NO+O₂ → 2NO₂ is second order in NO and first order in O₂. Complete the rate law for this reaction in the box below. Use the form k[A] [B]", where '1' 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 9.66 x 10³ M³s¹. Using this value for the rate constant, the rate of the reaction when [NO] 6.42 x 103 M and [0₂]- 3.01 x 103 M would be M/s.

The oxidation of nitrogen monoxide by oxygen at 25 °C 2NO+O₂ → 2NO₂ is second order in NO and first order in O₂. Complete the rate law for this reaction in the box below. Use the form k[A] [B]", where '1' 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 9.66 x 10³ M³s¹. Using this value for the rate constant, the rate of the reaction when [NO] 6.42 x 103 M and [0₂]- 3.01 x 103 M would be M/s.

Chemistry by OpenStax (2015-05-04)
Chemistry by OpenStax (2015-05-04)
1st Edition
ISBN:9781938168390
Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Publisher:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Chapter12: Kinetics
Section: Chapter Questions
Problem 25E: Nitrogen monoxide reacts with chlorine according to the equation: 2NOCI(g)2NOCI(g) The following...
See similar textbooks
icon
Related questions
Question
The oxidation of nitrogen monoxide by oxygen at 25 °C 2NO+O₂2NO₂ is second order in NO and first order in O₂. Complete the rate law for this reaction in the box below. Use the form k[A] [B]", where '1' 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 9.66 x 10³ M³s¹. Using this value for the rate constant, the rate of the reaction when [NO] = 6.42 x 10³ M and [0₂] =3.01 x 10³ M would be M/s.
Transcribed Image Text:The oxidation of nitrogen monoxide by oxygen at 25 °C 2NO+O₂2NO₂ is second order in NO and first order in O₂. Complete the rate law for this reaction in the box below. Use the form k[A] [B]", where '1' 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 9.66 x 10³ M³s¹. Using this value for the rate constant, the rate of the reaction when [NO] = 6.42 x 10³ M and [0₂] =3.01 x 10³ M would be M/s.
The reaction of mercury(II) chloride with oxalate ion 2HgCl₂ + C₂042 → 2C1+Hg₂ Cl₂ + 2C02 is first order in HgCl, and third order overall. Complete the rate law for this reaction in the box below. Use the form k[A] [B]", where '1' is understood for m or n and concentrations taken to the zero power do not appear. Don't enter 1 for m or n. Rate =
Transcribed Image Text:The reaction of mercury(II) chloride with oxalate ion 2HgCl₂ + C₂042 → 2C1+Hg₂ Cl₂ + 2C02 is first order in HgCl, and third order overall. Complete the rate law for this reaction in the box below. Use the form k[A] [B]", where '1' is understood for m or n and concentrations taken to the zero power do not appear. Don't enter 1 for m or n. Rate =
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
Rate Laws
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 by OpenStax (2015-05-04)
Chemistry by OpenStax (2015-05-04)
Chemistry
ISBN:
9781938168390
Author:
Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Publisher:
OpenStax
Chemistry: The Molecular Science
Chemistry: The Molecular Science
Chemistry
ISBN:
9781285199047
Author:
John W. Moore, Conrad L. Stanitski
Publisher:
Cengage Learning
Chemistry: Principles and Reactions
Chemistry: Principles and Reactions
Chemistry
ISBN:
9781305079373
Author:
William L. Masterton, Cecile N. Hurley
Publisher:
Cengage Learning
Chemistry for Engineering Students
Chemistry for Engineering Students
Chemistry
ISBN:
9781337398909
Author:
Lawrence S. Brown, Tom Holme
Publisher:
Cengage Learning
Chemistry: An Atoms First Approach
Chemistry: An Atoms First Approach
Chemistry
ISBN:
9781305079243
Author:
Steven S. Zumdahl, Susan A. Zumdahl
Publisher:
Cengage Learning
Chemistry
Chemistry
Chemistry
ISBN:
9781133611097
Author:
Steven S. Zumdahl
Publisher:
Cengage Learning
SEE MORE TEXTBOOKS