The emission of NO, by fossil fuel combustion can be prevented by injecting gaseous urea into the combustion mixture. The urea reduces NO (which oxidizes in air to form NO2) according to the reaction: 2 CO(NH;)»(3) + 4 NO(3) + O2(8) 4 Na(8) + 2 CO;(g) + 4 H¿O(g) Suppose that the exhaust stream of an automobile has a flow rate of 2.55 L/s at 655 Kand contains a partial pressure of NO of 12.4 torr. What total mass of urea is necessary to react complete- ly with the NO formed during 8.0 hours of driving?

The emission of NO, by fossil fuel combustion can be prevented by injecting gaseous urea into the combustion mixture. The urea reduces NO (which oxidizes in air to form NO2) according to the reaction: 2 CO(NH;)»(3) + 4 NO(3) + O2(8) 4 Na(8) + 2 CO;(g) + 4 H¿O(g) Suppose that the exhaust stream of an automobile has a flow rate of 2.55 L/s at 655 Kand contains a partial pressure of NO of 12.4 torr. What total mass of urea is necessary to react complete- ly with the NO formed during 8.0 hours of driving?

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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From the discussion question from Module 5, recall the chemical equation for the combustion of gasoline (iso-octane, C8H18) is: 2C8H18 + 25O2 ---> 16CO2 + 18H2O This means that 2 moles of iso-octane combine with 25 moles of CO2 to produce 16 moles of CO2 and 18 moles of water. This is important for understanding the impact of fossil fuel use on the atmosphere because burning one mole of fuel adds a lot of CO2. Thinking about this in terms of the stoichiometry, and change in concentration, suppose we had 1.0 mole of iso-octane dissolved in 1.0 m3 of atmosphere. That means the concentration of carbon-containing molecules would be 1 mole per cubic meter. However, ff we burned all that iso-octane and convert the C8H18 into CO2 the concentration of carbon-containing molecules increases. How much does the concentration of carbon-containing molecules increase if 1.0 mole of C8H18 in 1.0 m3 of air is converted into CO2 as shown in the chemical equation above?
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