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How many liters of HNO3 will be produced from 1.00 m³ of NH3 at STP, if the concentrated nitric acid solution contains 70 % (by mass) of HNO3. if the overall yield is 92.0%. Given: solution has density of 1.48 g/mL at STP _NH3(g) + ___O2(g) + ____H₂O(1)→ ____8HNO3(aq) + __H₂O(g) + ____NO(g) 2.67 L 1.76 L 3.67 O 7 from 1.67 L

How many liters of HNO3 will be produced from 1.00 m³ of NH3 at STP, if the concentrated nitric acid solution contains 70 % (by mass) of HNO3. if the overall yield is 92.0%. Given: solution has density of 1.48 g/mL at STP _NH3(g) + ___O2(g) + ____H₂O(1)→ ____8HNO3(aq) + __H₂O(g) + ____NO(g) 2.67 L 1.76 L 3.67 O 7 from 1.67 L

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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How many liters of HNO3 will be produced from 1.00 m³ of NH3 at STP, if the concentrated nitric acid solution contains 70 % (by mass) of HNO3. if the overall yield is 92.0 %. Given: solution has density of 1.48 g/mL at STP ___NH3(g) + ___O2(g) + ____H₂O(l) → _____8HNO3(aq) +____H₂O(g) + __NO(g) 2.67 L 1.76 L Ⓒ 3.67 fr 1.67 L
Transcribed Image Text:How many liters of HNO3 will be produced from 1.00 m³ of NH3 at STP, if the concentrated nitric acid solution contains 70 % (by mass) of HNO3. if the overall yield is 92.0 %. Given: solution has density of 1.48 g/mL at STP ___NH3(g) + ___O2(g) + ____H₂O(l) → _____8HNO3(aq) +____H₂O(g) + __NO(g) 2.67 L 1.76 L Ⓒ 3.67 fr 1.67 L
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