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The industrial production of nitric acid (HNO3) is a multistep process. The first step is the oxidation of ammonia (NH3) over a catalyst with excess oxygen (O2) to produce nitrogen monoxide (NO) gas as shown by the unbalanced equation given here: Part A What volume of O, at 798 mmHg and 33 °C is required to synthesize 20.0 mol of NO? Express your answer numerically in litres. ?NH3(9)+?O2(9)–+?NO(9)+?H¿O(g) • View Available Hint(s) volume of O, = 598 L Submit Previous Answers v Correct Correct answer is shown. Your answer 598.2 L was either rounded differently or used a different number of significant figures than required for this part. You have calculated the theoretical volume of O, needed to produce 20.0 mol of NO. However, in the industrial production of NO. oxygen is added in excess of this amount. Part B What volume of H2O(g) is produced by the reaction under the same conditions? Express your answer numerically in litres. > View Available Hint(s)

The industrial production of nitric acid (HNO3) is a multistep process. The first step is the oxidation of ammonia (NH3) over a catalyst with excess oxygen (O2) to produce nitrogen monoxide (NO) gas as shown by the unbalanced equation given here: Part A What volume of O, at 798 mmHg and 33 °C is required to synthesize 20.0 mol of NO? Express your answer numerically in litres. ?NH3(9)+?O2(9)–+?NO(9)+?H¿O(g) • View Available Hint(s) volume of O, = 598 L Submit Previous Answers v Correct Correct answer is shown. Your answer 598.2 L was either rounded differently or used a different number of significant figures than required for this part. You have calculated the theoretical volume of O, needed to produce 20.0 mol of NO. However, in the industrial production of NO. oxygen is added in excess of this amount. Part B What volume of H2O(g) is produced by the reaction under the same conditions? Express your answer numerically in litres. > View Available Hint(s)

Chemistry
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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Part B please

I Review | Constants | Periodic Table The industrial production of nitric acid (HNO3) is a multistep process. The first step is the oxidation of ammonia (NH3) over a catalyst with excess oxygen (O2) to produce nitrogen monoxide (NO) gas as shown by the unbalanced equation given here: Part A What volume of 02 at 798 mmHg and 33 °C is required to synthesize 20.0 mol of NO? Express your answer numerically in litres. ?NH3(9)+?O2 (9)–→?NO(g)+?H2O(g) • View Available Hint(s) volume of O, = 598 L Submit Previous Answers v Correct Correct answer is shown. Your answer 598.2 L was either rounded differently or used a different number of significant figures than required for this part. You have calculated the theoretical volume of O2 needed to produce 20.0 mol of NO. However, in the industrial production of NO, oxygen is added in excess of this amount. Part B What volume of H2O(g) is produced by the reaction under the same conditions? Express your answer numerically in litres. • View Available Hint(s) Πν ΑΣφ ? volume of H2O = L Submit
Transcribed Image Text:I Review | Constants | Periodic Table The industrial production of nitric acid (HNO3) is a multistep process. The first step is the oxidation of ammonia (NH3) over a catalyst with excess oxygen (O2) to produce nitrogen monoxide (NO) gas as shown by the unbalanced equation given here: Part A What volume of 02 at 798 mmHg and 33 °C is required to synthesize 20.0 mol of NO? Express your answer numerically in litres. ?NH3(9)+?O2 (9)–→?NO(g)+?H2O(g) • View Available Hint(s) volume of O, = 598 L Submit Previous Answers v Correct Correct answer is shown. Your answer 598.2 L was either rounded differently or used a different number of significant figures than required for this part. You have calculated the theoretical volume of O2 needed to produce 20.0 mol of NO. However, in the industrial production of NO, oxygen is added in excess of this amount. Part B What volume of H2O(g) is produced by the reaction under the same conditions? Express your answer numerically in litres. • View Available Hint(s) Πν ΑΣφ ? volume of H2O = L Submit
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