Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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On Easter Sunday, April 3, 1983, nitric acid spilled from a tank car near downtown Denver, Colorado. The spill was neutralized with sodium carbonate:
2 HNO3 (aq) + Na2CO3 (s) --> 2 NaNO3 (aq) + H2O (l) + CO2 (g)
Calculate ΔH° for this reaction. Approximately 2.0 x 104 gal nitric acid was spilled. Assume that the acid was an aqueous solution containing 70.0% HNO3 by mass with a density of 1.42 g cm-3. How much sodium carbonate was required for complete neutralization of the spill, and how much heat was evolved? [ΔHf° for NaNO3(aq) = -467 kJ/mol]
According to The Denver Post for April 4, 1983, authorities feared that dangerous air pollution might occur during the neutralization. Considering the magnitude of ΔH°, what was their major concern?
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