Assume that the acid was an aqueous solution containing 80.0% HNO3 by mass with a density of 1.42 g/cm3. How much sodium carbonate was required for complete neutralization of the spill?
On Easter Sunday, April 23, 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 ?H° for this reaction. kJ Approximately 5.0 10^4 gal nitric acid was spilled. Assume that the acid was an aqueous solution containing 80.0% HNO3 by mass with a density of 1.42 g/cm3. How much sodium carbonate was required for complete neutralization of the spill? (?Hf° for NaNO3(aq) = -467 kJ/mol.) g How much heat was evolved? kJ According to The Denver Post for April 4,1983, authorities feared that dangerous air pollution might occur during the neutralization. Considering the magnitude of ?H°, what was their major concern?
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