Reaction of nitrogen monoxide and hydrogen A student collects the data below for the reaction: 2 NO(g) + 2 H2(g) → N2(g) + 2 H2O(g) Trial [NO]i [H2]i Initial Rate (M/s) 1 0.050 M 0.050 M 0.0917 2 0.10 M 0.050 M 0.367 3 0.10 M 0.10 M 0.734 Determine the rate law for the reaction. multiple choice 1.Rate = k[NO][H2] 2.Rate = k[NO]4[H2]2 3.Rate = k[NO]2[H2]2 4.Rate = k[NO]2[H2] 5.The rate law cannot be determined from the given information.
Reaction of nitrogen monoxide and hydrogen A student collects the data below for the reaction: 2 NO(g) + 2 H2(g) → N2(g) + 2 H2O(g) Trial [NO]i [H2]i Initial Rate (M/s) 1 0.050 M 0.050 M 0.0917 2 0.10 M 0.050 M 0.367 3 0.10 M 0.10 M 0.734 Determine the rate law for the reaction. multiple choice 1.Rate = k[NO][H2] 2.Rate = k[NO]4[H2]2 3.Rate = k[NO]2[H2]2 4.Rate = k[NO]2[H2] 5.The rate law cannot be determined from the given information.
Chemistry for Engineering Students
4th Edition
ISBN:9781337398909
Author:Lawrence S. Brown, Tom Holme
Publisher:Lawrence S. Brown, Tom Holme
Chapter11: Chemical Kinetics
Section: Chapter Questions
Problem 11.98PAE: Experiments show that the reaction of nitrogen dioxide with fluorine, 2 NO2(g) + F2(g) —* 2 FNO2(g)...
Related questions
Question
Reaction of nitrogen monoxide and hydrogen
A student collects the data below for the reaction:
2 NO(g) + 2 H2(g) → N2(g) + 2 H2O(g)
| Trial | [NO]i | [H2]i | Initial Rate (M/s) |
| 1 | 0.050 M | 0.050 M | 0.0917 |
| 2 | 0.10 M | 0.050 M | 0.367 |
| 3 | 0.10 M | 0.10 M | 0.734 |
Determine the rate law for the reaction.
multiple choice
1.Rate = k[NO][H2]
2.Rate = k[NO]4[H2]2
3.Rate = k[NO]2[H2]2
4.Rate = k[NO]2[H2]
5.The rate law cannot be determined from the given information.
Expert Solution
Step 1
If we look at the trial 1 and 2, the concentration of A is doubled and B remains same. So, on doubling the concentration of A, the rate becomes 4 times of the initial rate. That is 0.0917 becomes 4×0.0917 = 0.367.
Hence the order of reaction with respect to A is 2.
Step 2
If we look at the trial 2 and 3, the concentration of B is doubled and A remains same. So, on doubling the concentration of B, the rate becomes 2 times of the initial rate. That is 0.367 becomes 2×0.367 = 0.734.
Hence the order of the reacton with respect to B is 1.
Step by step
Solved in 4 steps
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.Recommended textbooks for you
Chemistry for Engineering Students
Chemistry
ISBN:
9781337398909
Author:
Lawrence S. Brown, Tom Holme
Publisher:
Cengage Learning
Chemistry & Chemical Reactivity
Chemistry
ISBN:
9781133949640
Author:
John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:
Cengage Learning
Chemistry & Chemical Reactivity
Chemistry
ISBN:
9781337399074
Author:
John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:
Cengage Learning
Chemistry for Engineering Students
Chemistry
ISBN:
9781337398909
Author:
Lawrence S. Brown, Tom Holme
Publisher:
Cengage Learning
Chemistry & Chemical Reactivity
Chemistry
ISBN:
9781133949640
Author:
John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:
Cengage Learning
Chemistry & Chemical Reactivity
Chemistry
ISBN:
9781337399074
Author:
John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:
Cengage Learning
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
ISBN:
9781285199047
Author:
John W. Moore, Conrad L. Stanitski
Publisher:
Cengage Learning
Chemistry: Matter and Change
Chemistry
ISBN:
9780078746376
Author:
Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom
Publisher:
Glencoe/McGraw-Hill School Pub Co