A 32.7 L cylinder of a gas used for calibration of blood gas analyzers in medical laboratories contains 216 g CO2, 696 g 02, and 5854 g N2. The gas is kept at 25.0°C. You may assume that this is an ideal gas. What is the partial pressure of CO2 in this container? atm What is the total pressure of gases in this container? atm

A 32.7 L cylinder of a gas used for calibration of blood gas analyzers in medical laboratories contains 216 g CO2, 696 g 02, and 5854 g N2. The gas is kept at 25.0°C. You may assume that this is an ideal gas. What is the partial pressure of CO2 in this container? atm What is the total pressure of gases in this container? atm

Chemistry & Chemical Reactivity

10th Edition

ISBN:9781337399074

Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Chapter10: Gases And Their Properties

Section: Chapter Questions

Problem 38PS: A cylinder of compressed gas is labeled Composition (mole %): 4.5% H2S, 3.0% CO2, balance N2. The...

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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.
A cylinder of compressed gas is labeled Composition (mole %): 4.5% H2S, 3.0% CO2, balance N2. The pressure gauge attached to the cylinder reads 46 atm. Calculate the partial pressure of each gas, in atmospheres, in the cylinder.
A typical barometric pressure in Redding. California, is about 750 mm Hg. Calculate this pressure in atm and kPa.
You have a gas, one of the three known phosphorus-fluorine compounds (PF3, PF3, and P2F4). To find out which, you have decided to measure its molar mass. (a) First, yon determine that the density of the gas is 5.60 g/L at a pressure of 0.971 atm and a temperature of 18.2 C. Calculate the molar mass and identify the compound. (b) To check the results from part (a), you decide to measure the molar mass based on the relative rales of effusion of the unknown gas and CO2. You find that CO2 effuses at a rate of 0.050 mol/min, whereas the unknown phosphorus fluoride effuses at a rate of 0.028 mol/min. Calculate the molar mass of the unknown gas based on these results.
In the Mthode Champenoise, grape juice is fermented in a wine bottle to produce sparkling wine. The reaction is C6H12O6(aq)2C2H5OH(aq)+2CO2(g) Fermentation of 750. mL grape juice (density = 1.0 g/cm3) is allowed to take place in a bottle with a total volume of 825 mL until 12% by volume is ethanol (C2H5OH). Assuming that the CO2 is insoluble in H2O (actually, a wrong assumption), what would be the pressure of CO2 inside the wine bottle at 25C? (The density of ethanol is 0.79 g/cm3.)
You have a 550.-mL tank of gas with a pressure of 1.56 atm at 24 C. You thought the gas was pure carbon monoxide gas, CO, but you later found it was contaminated by small quantities of gaseous CO2 and O2. Analysis shows that the tank pressure is 1.34 atm (at 24 C) if the CO2 is removed. Another experiment shows that 0.0870 g of O2 can be removed chemically. What are the masses of CO and CO2 in the tank, and what is the partial pressure of each of the three gases at 25 C?
93 The complete combustion of octane can be used as a model for the burning of gasoline: 2C8H18+25O216CO2+18H2O Assuming that this equation provides a reasonable model of the actual combustion process, what volume of air at 1.0 atm and 25°C must be taken into an engine to burn 1 gallon of gasoline? (The partial pressure of oxygen in air is 0.21 atm and the density of liquid octane is 0.70 g/mL.)
A study of climbers who reached the summit of Mount Everest without supplemental oxygen showed that the partial pressures of O2 and CO2 in their lungs were 35 mm Mg and 7.5 mm Hg, respectively. The barometric pressure at the summit was 253 mm Hg. Assume the lung gases are saturated with moisture at a body temperature of 37 C [which means the partial pressure of water vapor in the lungs is P(H2O) = 47.1 mm Hg]. If you assume the lung gases consist of only O2, N2, CO2, and H2O, what is the partial pressure of N2?