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

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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