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How does the rate of decomposition vary over time? The compound dinitrogen pentoxide (N,O5) decomposes in air according to the equation Time (min) [N,0,] (mol/L) 0.01756 20.0 0.00933 2N,Os(g) → 4NO2(g) + O2(g) 40.0 0.00531 60.0 0.00295 Knowing the rate of decomposition allows its concentration to be determined at any time. 80.0 0.00167 100.0 0.00094 Analysis The table shows the results of an experiment in which the concentration of N,Os, was measured over time at normal atmospheric pressure and a temperature of 45°C. 2. Express the average reaction rate for each time interval in moles of NO2 produced per liter per minute. Use the reaction equation to explain the relationship between these rates and those calculated in Question 1. Think Critically 1. Calculate the average reaction rate for each time interval: 0-20 min, 40-60 min, and 80-100 min. Express each rate as a positive number and in moles of N205 consumed per liter per minute. 3. Interpret the data and your calculations in describing how the average rate of decomposition of N205 varies over time. 4. Apply collision theory to infer why the reaction rate varies as it does.

How does the rate of decomposition vary over time? The compound dinitrogen pentoxide (N,O5) decomposes in air according to the equation Time (min) [N,0,] (mol/L) 0.01756 20.0 0.00933 2N,Os(g) → 4NO2(g) + O2(g) 40.0 0.00531 60.0 0.00295 Knowing the rate of decomposition allows its concentration to be determined at any time. 80.0 0.00167 100.0 0.00094 Analysis The table shows the results of an experiment in which the concentration of N,Os, was measured over time at normal atmospheric pressure and a temperature of 45°C. 2. Express the average reaction rate for each time interval in moles of NO2 produced per liter per minute. Use the reaction equation to explain the relationship between these rates and those calculated in Question 1. Think Critically 1. Calculate the average reaction rate for each time interval: 0-20 min, 40-60 min, and 80-100 min. Express each rate as a positive number and in moles of N205 consumed per liter per minute. 3. Interpret the data and your calculations in describing how the average rate of decomposition of N205 varies over time. 4. Apply collision theory to infer why the reaction rate varies as it does.

Chemistry & Chemical Reactivity
Chemistry & Chemical Reactivity
9th Edition
ISBN:9781133949640
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Chapter14: Chemical Kinetics: The Rates Of Chemical Reactions
Section: Chapter Questions
Problem 6PS: 6. Phenyl acetate, an ester, reacts with water according to the equation The data in the table were...
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PROBLEM-SOLVING LAB Interpret Data How does the rate of decomposition vary over time? The compound dinitrogen pentoxide (N,O5) decomposes in air according to the equation Time (min) [N,0,] (mol/L) 0.01756 20.0 0.00933 2N,Os(g) → 4NO2(g) + O2(g) 40.0 0.00531 60.0 0.00295 Knowing the rate of decomposition allows its concentration to be determined at any time. 80.0 0.00167 100.0 0.00094 Analysis The table shows the results of an experiment in which the concentration of N205, was measured over time at normal atmospheric pressure and a temperature of 45°C. 2. Express the average reaction rate for each time interval in moles of NO2 produced per liter per minute. Use the reaction equation to explain the relationship between these rates and those calculated in Question 1. Think Critically 1. Calculate the average reaction rate for each time interval: 0-20 min, 40-60 min, and 80-100 min. Express each rate as a positive number and in moles of N2O5 consumed per liter per minute. 3. Interpret the data and your calculations in describing how the average rate of decomposition of N2O5 varies over time. 4. Apply collision theory to infer why the reaction rate varies as it does.
Transcribed Image Text:PROBLEM-SOLVING LAB Interpret Data How does the rate of decomposition vary over time? The compound dinitrogen pentoxide (N,O5) decomposes in air according to the equation Time (min) [N,0,] (mol/L) 0.01756 20.0 0.00933 2N,Os(g) → 4NO2(g) + O2(g) 40.0 0.00531 60.0 0.00295 Knowing the rate of decomposition allows its concentration to be determined at any time. 80.0 0.00167 100.0 0.00094 Analysis The table shows the results of an experiment in which the concentration of N205, was measured over time at normal atmospheric pressure and a temperature of 45°C. 2. Express the average reaction rate for each time interval in moles of NO2 produced per liter per minute. Use the reaction equation to explain the relationship between these rates and those calculated in Question 1. Think Critically 1. Calculate the average reaction rate for each time interval: 0-20 min, 40-60 min, and 80-100 min. Express each rate as a positive number and in moles of N2O5 consumed per liter per minute. 3. Interpret the data and your calculations in describing how the average rate of decomposition of N2O5 varies over time. 4. Apply collision theory to infer why the reaction rate varies as it does.
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