Concentrated nitric acid acts on copper to give nitrogen dioxide and dissolved copper ions (Fig. 9.11) according to the balanced chemical equation: Cu(s) + 4 H* (aq) +2 NO3¯(aq) → 2 NO2(g) + Cu²+(aq) + 2 HzO(€) Suppose that 6.80 g copper is consumed in this reaction, and that the NO, is collected at a pressure of 0.970 atm and a temperature of 45°C. Calculate the volume of NO, produced.
Concentrated nitric acid acts on copper to give nitrogen dioxide and dissolved copper ions (Fig. 9.11) according to the balanced chemical equation: Cu(s) + 4 H* (aq) +2 NO3¯(aq) → 2 NO2(g) + Cu²+(aq) + 2 HzO(€) Suppose that 6.80 g copper is consumed in this reaction, and that the NO, is collected at a pressure of 0.970 atm and a temperature of 45°C. Calculate the volume of NO, produced.
Chemistry: The Molecular Science
5th Edition
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter10: Fuels, Organic Chemicals, And Polymers
Section: Chapter Questions
Problem 89QRT
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