Homework Help is Here – Start Your Trial Now!
Science
Chemistry
The first-order rate constant for the decomposition of NjOs, given below, at 70°C is 6.82 x 10s. Suppose we start with 0.0150 mol of N₂O(g) in a volume of 1.0 L 2 N₂O5(0)4 NO₂(g) + O₂(g) (a) How many moles of N,O, will remain after 3.0 min? 0.004 X mol (b) How many minutes will it take for the quantity of No, to drop to 0.005 mol? 2.68 ✔min (c) What is the half-life of N.O, at 70 C7 101.0 x min

The first-order rate constant for the decomposition of NjOs, given below, at 70°C is 6.82 x 10s. Suppose we start with 0.0150 mol of N₂O(g) in a volume of 1.0 L 2 N₂O5(0)4 NO₂(g) + O₂(g) (a) How many moles of N,O, will remain after 3.0 min? 0.004 X mol (b) How many minutes will it take for the quantity of No, to drop to 0.005 mol? 2.68 ✔min (c) What is the half-life of N.O, at 70 C7 101.0 x min

Chemistry: Principles and Reactions
Chemistry: Principles and Reactions
8th Edition
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:William L. Masterton, Cecile N. Hurley
Chapter11: Rate Of Reaction
Section: Chapter Questions
Problem 42QAP: The decomposition of sulfuryl chlorideSO2Cl2fur dioxide and chlorine gases is a first-order...
See similar textbooks
icon
Related questions
Question
Please provide only typed answer solution no handwritten solution needed
The first-order rate constant for the decomposition of Njos, given below, at 70°C is 6.82 x 10 s¹. Suppose we start with 0.0150 mol of NO(g) in a volume of 1.0L 2 N₂0 (0) 4 NO₂(g) + O₂(g) (a) How many moles of N,O, will remain after 3.0 min? 0.004 X mol (b) How many minutes will it take for the quantity of N₂0, to drop to 0.005 mol? 12.68 ✓min (c) What is the half-life of N,O, at 20°C 101.0 x min
Transcribed Image Text:The first-order rate constant for the decomposition of Njos, given below, at 70°C is 6.82 x 10 s¹. Suppose we start with 0.0150 mol of NO(g) in a volume of 1.0L 2 N₂0 (0) 4 NO₂(g) + O₂(g) (a) How many moles of N,O, will remain after 3.0 min? 0.004 X mol (b) How many minutes will it take for the quantity of N₂0, to drop to 0.005 mol? 12.68 ✓min (c) What is the half-life of N,O, at 20°C 101.0 x min
Molecular iodine, 1₂(g), dissociates into iodine atoms at 625 K with a first-order rate constant of 0.271 s (a) What is the half-life for this reaction? 2.56 (b) If you start with 0.046 M 1₂ at this temperature, how much will remain after 5.17 s assuming that the iodine atoms do not recombine to form 1,? 0.011 XM D
Transcribed Image Text:Molecular iodine, 1₂(g), dissociates into iodine atoms at 625 K with a first-order rate constant of 0.271 s (a) What is the half-life for this reaction? 2.56 (b) If you start with 0.046 M 1₂ at this temperature, how much will remain after 5.17 s assuming that the iodine atoms do not recombine to form 1,? 0.011 XM D
Expert Solution
steps

Step by step

Solved in 7 steps

SEE SOLUTIONCheck out a sample Q&A here
Blurred answer
Knowledge Booster
Reaction Rates
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
Recommended textbooks for you
Chemistry: Principles and Reactions
Chemistry: Principles and Reactions
Chemistry
ISBN:
9781305079373
Author:
William L. Masterton, Cecile N. Hurley
Publisher:
Cengage Learning
Chemistry: The Molecular Science
Chemistry: The Molecular Science
Chemistry
ISBN:
9781285199047
Author:
John W. Moore, Conrad L. Stanitski
Publisher:
Cengage Learning
Chemistry for Engineering Students
Chemistry for Engineering Students
Chemistry
ISBN:
9781337398909
Author:
Lawrence S. Brown, Tom Holme
Publisher:
Cengage Learning
Chemistry: Principles and Practice
Chemistry: Principles and Practice
Chemistry
ISBN:
9780534420123
Author:
Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:
Cengage Learning
Chemistry & Chemical Reactivity
Chemistry & Chemical Reactivity
Chemistry
ISBN:
9781337399074
Author:
John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:
Cengage Learning
Chemistry & Chemical Reactivity
Chemistry & Chemical Reactivity
Chemistry
ISBN:
9781133949640
Author:
John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:
Cengage Learning
SEE MORE TEXTBOOKS