Please don't provide handwritten solution .... Carbon tetrachloride can be used to make CFC-12, CF2Cl2, and CFC-11, CFCI 3:3 HF(g) + 2 CCl4(g) → CF2Cl2(g) + CFCI 3(g) + 3 HCl(g)(a) What is the minimum volume of HF(g) in cubic meters at 1.3 atm and 17°C that would be necessary to react 218 kg CCI4 in this reaction?4.0✓m3(b) What is the maximum volume of CFC-12 at 763 mmHg and 17°C that can be formed from 726 m³ of hydrogen fluoride gas at 1405 mmHg and 27°C?m34.0Supporting Materials

To solve this problem, we can use the ideal gas law equation PV=nRT to find the number of moles of…

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Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter6: The Gaseous State

Section: Chapter Questions

Problem 6.57QE

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A sample of natural gas is 85.2% methane, CH4, and 14.8% ethane, C2H6, by mass. What is the density of this mixture at 18C and 771 mmHg?
Ethanol, the alcohol used in automobile fuels, is produced by the fermentation of sugars present in plants. Corn is often used as the sugar source. The following equation represents the fermentation of glucose, the sugar in corn, by yeast to produce ethanol and carbon dioxide. C6H12O6(aq)2C2H5OH(aq)+2CO2(g) Ethanol is combusted in an automobile engine according to the equation C2H5OH(l)+3O2(g)2CO2(g)+3H2O(g) What would be the total volume of CO2 gas formed at STP when 3.00 kg of sugar is fermented and the ethanol is then combusted in an automobile engine?
5-114 Carbon dioxide gas, saturated with water vapor, can be produced by the addition of aqueous acid to calcium carbonate based on the following balanced net ionic equation: (a) How many moles of wet CO (g), collected at 60.°C and 774 torr total pressure, are produced by the complete reaction of 10.0 g of CaCO3 with excess acid? (b) What volume does this wet CO2 occupy? (c) What volume would the CO2 occupy at 774 torr if a desiccant (a chemical drying agent) were added to remove the water? The vapor pressure of water at 60.°C is 149.4 mm Hg.
A 21.4-mL volume of hydrochloric acid reacts completely with a solid sample of MgCO3. The reaction is 2HCl(aq)+MgCO3(s)CO2(g)+H2O(l)+MgCl2(aq) The volume of CO2 formed is 159 mL at 23C and 731 mmHg. What is the molarity of the HCl solution?
Many nitrate salts can be decomposed by heating. For example, blue, anhydrous copper(II) nitrate produces the gases nitrogen dioxide and oxygen when heated. In the laboratory, you find that a sample of this salt produced a 0.195-g mixture of gaseous NO2 and O2 with a total pressure of 725 mm Hg at 35 C in a 125-mL flask (and black, solid CuO was left as a residue). What is the average molar mass of the gas mixture? What are the mole fractions of NO2 and O2 in the mixture? What amount of each gas b in the mixture? Do these amounts reflect the relative amounts of NO2 and O2 expected based on the balanced equation? Is it possible that the fact that some NO2 molecules combine to give N2O4 plays a role? Heating copper(II) nitrate produces nitrogen dioxide and oxygen gas and leaves a residue of copper(ll) oxide.
109 An ore sample with a mass of 670 kg contains 27.7% magnesium carbonate, MgCO3. If all of the magnesium carbonate in this ore sample is decomposed to form carbon dioxide, describe how to determine what volume of CO2 is evolved during the process. What would have to be measured to predict the needed volume in advance?
A person exhales about 5.8 102 L of carbon dioxide per day (at STP). The carbon dioxide exhaled by an astronaut is absorbed from the air of a space capsule by reaction with lithium hydroxide, LiOH. 2LiOH(s)+CO2(g)Li2CO3(s)+H2O(l) How many grams of lithium hydroxide are required per astronaut per day?
As 1 g of (lie radioactive element radium decays over 1 year. k produces 1.161018 alpha particles (helium nuclei). Each alpha particle becomes an atom of helium gas. What is the pressure ¡n pascal of the helium gas produced if it occupies a volume of 125 mL at a temperature of 25 C?
Hydrogen gas is used in weather balloon because it is less expensive than Helium. Assume that 5.57 g of H2 is used to fill a weather balloon to an initial volume of 67 L at 1.04 atm. If the ballloon rises to an altitude where the pressure is 0.047 atm, what is its new volume? Assume that the temperature remains constant.
Hyperbaric oxygen therapy is used to treat patients with carbon monoxide poisoning as well as to treat divers with the bends. In hyperbaric oxygen therapy, a patient is placed inside a 7.0-ft cylinder with a 3.0-ft diameter, which is then filled with oxygen gas to a total pressure of 2.50 atm. Assuming the patient takes up 32.0% of the chambers volume , what volume of O2(g) from a gas cylinder at 25 C and 95 atm is required to fill the chamber to a total pressure of 2.50 atm at 25 C7 Assume the hyperbaric chamber initially contains air at 1.00 atm before O2(g) is added.
If equal masses of O2 and N2 are placed in separate containers of equal volume at the same temperature, which of the following statements is true? If false, explain why it is false. (a) The pressure in the flask containing N2 is greater than that in the flask containing O2. (b) There are more molecules in the flask containing O2 than in the flask containing N2.
Raoul Pictet, the Swiss physicist who first liquefied oxygen, attempted to liquefy hydrogen. He heated potassium formate, KCHO2, with KOH in a closed 2.50-Lvessel. KCHO2(s)+KOH(s)K2CO3(s)+H2(g) If 75.0 g of potassium formate reacts in a 2.50-L vessel, which was initially evacuated, what pressure of hydrogen will be attained when the temperature is finally cooled to 25C? Use the preceding chemical equation and ignore the volume of solid product.

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