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? ?NH3(9)+?O2(g)→?NO(g)+?H2O(g) 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 02 at 798 mmHg and 33 °C is required to synthesize 20.0 mol of NO? ?NH3(9)+?O2(g)→?NO(g)+?H2O(g) Express your answer numerically in litres. • View Available Hint(s)

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...

See similar textbooks

Similar questions

5.72 A sample of zinc metal reacts completely with an excess of hydrochloric acid: Zn(s) + 2HCl(aq) → ZnCl₂(aq) + H₂(g) The hydrogen gas produced is collected over water at 25.0°C using an arrangement similar to that shown in Figure 5.15. The volume of the gas is 7.80 L, and the pressure is 0.980 atm. Calculate the amount of zinc metal in grams consumed in the reaction. (Vapor pressure of water at 25°C = 23.8 mmHg.)
A reaction of 0.028 g of magnesium with excess hydrochloric acid generated 31.0 mL of hydrogen gas. The gas was collected by water displacement in a 22 °C water bath. The barometric pressure in the lab during the experiment was 746 mm Hg. What is the theoretical amount (mol) of hydrogen gas that should have formed from the reaction of 0.028 grams of magnesium with an excess of hydrochloric acid? ??(?) + 2???(??) → ????2(??) + ?2(?)
Please don't provide handwritten solution
Sometimes in Io we collect the gas formed by a chemical reaction over water (see sketch at right). This makes it easy to isolate and measure the amount of gas produced. collected gas Suppose the O, gas evolved by a certain chemical reaction taking place at 30.0 °C is collected over water, using chemical reaction water an apparatus something like that in the sketch, and the final volume of gas in the collection tube is measured to be 44.8 mL. Sketch of a gas-collection apparatus ab Calculate the mass of O, that is in the collection tube. Round your answer to 2 significant digits. You can make any normal and reasonable assumption about the reaction conditions and the nature of the gases. Explanation Check O 2022 McGraw Hill LLC. All Rights Reserved. Terms of Use I Privacy Center | Accessibility 6:20 AM N 35°F Mostly cloudy ENG 1/23/2022 Pll 26 506 F90 T. 4. R] T Y D F
A small amount of oxygen gas may be prepared in the laboratory by the decomposition of potassium chlorate, KClO3, according to the following equation: 2KClO3(s)  2KCl(s) + 3O2(g) A 1.54-g sample of KClO3 is completely decomposed and the oxygen gas produced is collected over water at 25oC and at a total pressure of 757.0 torrs. (a) If the vapor pressure of water at 25oC is 23.8 torr, what is the partial pressure of O2 collected? (b) How many milliliters (mL) of O2 gas are collected under the stated condition? What is the volume of O2 gas if collected at STP?
Please refer to photo! Thanks!
Hand written solutions are strictly prohibited.
please help me with this chemistry ques. And show all your work
The balanced equation for the decomposition of potassium chlorate is shown below. When carried out in lab, this reaction is found to produce 340 mL of oxygen gas at STP. For your convenience, the molar mass of each substance is shown below their formulas (in purple). Use this information to make the requested calculation: 2 KCIO3(s) -> 2 KCI(s) + 3 02(g) 122.551 74.551 32 Determine the percent yield if the reaction consumes 2300 mg of potassium chlorate:
10
19. A 2.00 liter of sample of ethane, C;H6, is burned at 1.00 atm and 25.0 °C with 1.50 liters of oxygen. What is the mass of water vapor will be produced from the burning of ethane? What would be the volume of the water vapor under the same conditions? (Hint: determine the limiting reagent!) (m = 1.96 g; v = 1.29 L.