The industrial production of nitric acid (HNO3) is a multistep process.The first step is the oxidation of ammonia (NH3) over a catalyst withexcess oxygen (O2) to produce nitrogen monoxide (NO) gas asshown by the unbalanced equation given here:Part A?NH3(9)+?O2(9)–→?NO(g)+?H2O(g)What volume of O, at 722 mmHg and 21 °Cis required to synthesize 22.5 mol of NO?Express your answer numerically in litres.• View Available Hint(s)volume of O, =SubmitPrevious Answers Request Answer

Given that: pressure, P = 722 mmHg = 722760= 0.95 atm temperature, T = 21 oC = 21 + 273 = 294 K…

Part A What volume of O2 at 722 mmHg and 21 °Cis required to synthesize 22.5 mol of NO? Express your answer numerically in litres. • View Available Hint(s) Πν ΑΣφ ? volume of O2 = L Submit Previous Answers Request Answer

Part A What volume of O2 at 722 mmHg and 21 °Cis required to synthesize 22.5 mol of NO? Express your answer numerically in litres. • View Available Hint(s) Πν ΑΣφ ? volume of O2 = L Submit Previous Answers Request Answer

Chemistry

9th Edition

ISBN:9781133611097

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

Chapter5: Gases

Section: Chapter Questions

Problem 161IP: In the presence of nitric acid, UO2+ undergoes a redox process. It is converted to UO22+ and nitric...

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