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: Principles and Practice
3rd Edition
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Chapter13: Chemical Kinetics
Section: Chapter Questions
Problem 13.23QE: Nitrogen monoxide reacts with chlorine to form nitrosyl chloride. NO(g)+12Cl2(g)NOCl(g) The figure...
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