A possible practical way to eliminate oxides of nitrogen (such as NO2) from automobile exhaust gases uses cyanuric acid, C3N3(OH)3. When heated to the relatively low temperature of 625°F, cyanuric acid converts to gaseous isocyanic acid (HNCO). Isocyanic acid reacts with NO2 in the exhaust to form nitrogen, carbon dioxide, and water, all of which are normal constituents of the air. (a) Write balanced equations for these two reactions. (b) If the process described earlier became practical, how much cyanuric acid (in kilograms) would be required to absorb the 1.7 × 1010 kg NO2 generated annually in auto exhaust in the United States?
A possible practical way to eliminate oxides of nitrogen (such as NO2) from automobile exhaust gases uses cyanuric acid, C3N3(OH)3. When heated to the relatively low temperature of 625°F, cyanuric acid converts to gaseous isocyanic acid (HNCO). Isocyanic acid reacts with NO2 in the exhaust to form nitrogen, carbon dioxide, and water, all of which are normal constituents of the air. (a) Write balanced equations for these two reactions. (b) If the process described earlier became practical, how much cyanuric acid (in kilograms) would be required to absorb the 1.7 × 1010 kg NO2 generated annually in auto exhaust in the United States?
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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A possible practical way to eliminate oxides of nitrogen (such as NO2) from automobile exhaust gases uses cyanuric acid, C3N3(OH)3. When heated to the relatively low temperature of 625°F, cyanuric acid converts to gaseous isocyanic acid (HNCO). Isocyanic acid reacts with NO2 in the exhaust to form nitrogen, carbon dioxide, and water, all of which are normal constituents of the air.
(a) Write balanced equations for these two reactions.
(b) If the process described earlier became practical, how much cyanuric acid (in kilograms) would be required to absorb the 1.7 × 1010 kg NO2 generated annually in auto exhaust in the United States?
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