12. The production of ammonia (NH3) is achieved industrially via the Haber-Bosch process, which consumes 1-2% of the world's energy supply each year. The reaction occurring is shown below: N2(g) + 3 H2(g) → 2 NH3(9) Suppose that 10.3 L of NH3(g) is collected at 573 K, with a total pressure of 75.72 atm by this process. The partial pressures of N2(g) and H2(g) in the same vessel are 16.09 atm and 48.27 atm, respectively. Show all of your work for full credit. a) What is the partial pressure (in atm) of ammonia gas in the sample? b) What is the mol fraction of ammonia gas? c) How many moles of ammonia gas are produced? d) How many liters of hydrogen gas must have reacted to produce this quantity of ammonia gas if the initial reaction vessel had a hydrogen pressure of 90.0 atm at 615 K?

12. The production of ammonia (NH3) is achieved industrially via the Haber-Bosch process, which consumes 1-2% of the world's energy supply each year. The reaction occurring is shown below: N2(g) + 3 H2(g) → 2 NH3(9) Suppose that 10.3 L of NH3(g) is collected at 573 K, with a total pressure of 75.72 atm by this process. The partial pressures of N2(g) and H2(g) in the same vessel are 16.09 atm and 48.27 atm, respectively. Show all of your work for full credit. a) What is the partial pressure (in atm) of ammonia gas in the sample? b) What is the mol fraction of ammonia gas? c) How many moles of ammonia gas are produced? d) How many liters of hydrogen gas must have reacted to produce this quantity of ammonia gas if the initial reaction vessel had a hydrogen pressure of 90.0 atm at 615 K?

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

A fuel cylinder for a camping stove contains 5.6 oz butane (C4H10), which produces 67.3 L of butane gas at 25 °C and 1.00 atm, if all of the butane in the fuel cylinder undergoes complete combustion. What volume of oxygen gas at 25 °C and 1.00 atm is needed to react with this amount of butane? L What volume of carbon dioxide gas at 25 °C and 1.00 atm is produced by this amount of butane? Question #7
As part of the production of vinyl chloride — which is used to make polyvinyl chloride (PVC) plastic — 1,2-dichloroethane, ClCH2CH2Cl, is decomposed to form vinyl chloride and hydrogen chloride. If 511 kg of 1,2-dichloroethane gas are released into a 97 m3 container, at what temperature will the pressure become 3.6 atm?
Sodium metal reacts with chlorine gas to form sodium chloride. A closed container of volume 2.00x10^3 ml contains chlorine gas at 27C and 1.25x10^4 torr. Then 3.90 g of solid sodium is introduced, and the reaction goes to completion. What is the final pressure (in atm) inside the container if the temperature rises to 47C.
A mixture of hydrogen and oxygen with a mole ratio of 2:1 is used to manufacture water according to the following reaction. 2H2(g) + O2(g) -> 2H2O(g) Before the reaction, the total pressure in the container at 25 degrees Celsius is 0.950 atm. Assuming a yield of 88.0% and no volume change, what is the final pressure in the container at 125 degrees after the reaction?
62.0 g of nitrogen at 100oC is in a 155.0 L container. How much nitrogen, in grams, must be removed to decrease the pressure by 10.5 mm Hg? (Assume the molar mass of N to be 14 g/mol).
In the the industrial synthesis of methanol from synthesis gas, gaseous carbon monoxide and hydrogen react via the appropriate catalysts to produce the gaseous product (balanced chemical equation below). C O ( g ) + 2 H 2 ( g ) → C H 3 O H ( g ) If the reactant gases are combined in a 1,703 L container at 247oC, and the initial partial pressures of CO and H2 are 11.7 atm and 14.4 atm, respectively, determine the maximum partial pressure of CH3OH that can be produced.
One method for preparing hydrogen gas is to pass HCl gas over hot aluminium: the other product of the reaction is AlCl3. If you wanted to use this reaction to fill a balloon with a volume of 28.500 L at sea level and a temperature of 25.5°C, what mass of aluminium would you need? What volume of HCl at STP would you need?
Roasting galena [lead(II) sulfide] is an early step in the industrial isolation of lead. How many liters of sulfur dioxide, measured at STP, are produced by the reaction of 6.45 kg of galena with 145. L of oxygen gas at 220 °C and 2.00 atm? Lead(II) oxide also forms. Be sure your answer has the correct number of significant figures. Note: Reference the Fundamental constants table for additional information. L SO₂ x10 X
22. A mercury manometer is used to measure pressure in the container illustrated. Calculate the pressure exerted by the gas if atmospheric pressure is 752 torr. P = 284 mm Hg
c) When coal is burnt, the sulphur present in coal is converted to sulphur dioxide which is responsible for the acid rain phenomenon. + O2 (g) → SO2 (g) (s) If 2.54 kg of sulphur is reacted with oxygen gas, determine the volume of sulphur dioxide gas formed at 30.5 °C and 851.2 mmHg.
A mixture of 3.1 grams of N2O and CH4 gases creates a pressure of 1140 mmHg at 270 ° C in a 2.46 liter container. What is the volume of CH4 gas in this container covered under normal conditions? (H = 1, C = 12, N = 14, O = 16)
Iron (III) oxide mined from the earth must be initially converted into the liquid metal before then being used in the formation of steel. The balanced reaction is given below. If 7.16 x 102 g of iron (III) oxide is reacted with excess carbon at a temperature of 2273 K, what volume of carbon dioxide gas, in liters, will be produced if the atmospheric pressure is 0.979 atm? 2 Fe2O3 (s) + 3 C (s) → 4 Fe (l) + 3 CO2 (g)