![Introductory Chemistry: A Foundation](https://www.bartleby.com/isbn_cover_images/9781337399425/9781337399425_largeCoverImage.gif)
Concept explainers
A tank contains a mixture of
![Check Mark](/static/check-mark.png)
Interpretation:
The partial pressure of oxygen and carbon dioxide gas should be calculated.
Concept Introduction:
Dalton’s law of partial pressure: In a container for mixture of gases, the total pressure is equal to the sum of partial pressures of all the gases present in the container. The partial pressure is the pressure exerted by a gas if it is the only gas present in the container.
Let a mixture of three gases with partial pressures
This is the Dalton’s law of partial pressure.
The behaviour of gases is assumed to be ideal thus, partial pressure of gases can be calculated from an ideal gas equation as follows:
Here, P is pressure, V is volume, n is number of moles, R is Universal gas constant and T is temperature of the gas.
The pressure exerted by an ideal gas depends on the number of gas particles, this does not depend on the nature of particles of gas. The two important things concluded from it will be:
- The volume of gases is important.
- The forces in between the particles of gas is not important.
Answer to Problem 69QAP
4.84 atm and 4.37 atm.
Explanation of Solution
Calculation:
First calculate the number of moles of each gas as follows:
Since, molar mass of O2 is 32 g/mol thus, number of moles will be:
Similarly, molar mass of
Thus, total number of moles will be:
Putting the values,
From total pressure and number of moles, volume can be calculated using the ideal gas equation as follows:
First convert the temperature from
Thus,
Putting the values,
Thus,
Now from volume, partial pressure of gases can be calculated from ideal gas equation as follows:
Putting the values,
Similarly, partial pressure of
Putting the values,
Thus, partial pressure of oxygen and carbon dioxide gas is 4.84 atm and 4.37 atm respectively.
Want to see more full solutions like this?
Chapter 13 Solutions
Introductory Chemistry: A Foundation
- Given that a sample of air is made up of nitrogen, oxygen, and argon in the mole fractions 0.78 N2, 0.21 O2, and 0.010 Ar, what is the density of air at standard temperature and pressure?arrow_forwardYou have an equimolar mixture of the gases SO2 and O2, along with some He, in a container fitted with a piston. The density of this mixture at STP is 1.924 g/L. Assume ideal behavior and constant temperature and pressure. a. What is the mole fraction of He in the original mixture? b. The SO2 and O2 react to completion to form SO3. What is the density of the gas mixture after the reaction is complete?arrow_forward93 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.)arrow_forward
- The density of air 20 km above Earths surface is 92 g/m3. The pressure of the atmosphere is 42 mm Hg, and the temperature is 63 C. (a) What is the average molar mass of the atmosphere at this altitude? (b) If the atmosphere at this altitude consists of only O2 and N2, what is the mole fraction of each gas?arrow_forwardYou have two pressure-proof steel cylinders of equal volume, one containing 1.0 kg of CO and the other containing 1.0 kg of acetylene, C2H2. (a) In which cylinder is the pressure greater at 25 C? (b) Which cylinder contains the greater number of molecules?arrow_forwardSulfur trioxide, SO3, is produced in enormous quantities each year for use in the synthesis of sulfuric acid. S(s)+O2(g)SO2(g)2SO2(g)+O2(g)2SO3(g) What volume of O2(g) at 350.C and a pressure of 5.25 atm is needed to completely convert 5.00 g sulfur to sulfur trioxide?arrow_forward
- 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.arrow_forwardYou 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.arrow_forwardIf 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.arrow_forward
- Chemistry: Matter and ChangeChemistryISBN:9780078746376Author:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl WistromPublisher:Glencoe/McGraw-Hill School Pub CoChemistry & Chemical ReactivityChemistryISBN:9781337399074Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage LearningChemistry & Chemical ReactivityChemistryISBN:9781133949640Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage Learning
- Chemistry: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher:Cengage LearningChemistry for Engineering StudentsChemistryISBN:9781337398909Author:Lawrence S. Brown, Tom HolmePublisher:Cengage LearningChemistry: An Atoms First ApproachChemistryISBN:9781305079243Author:Steven S. Zumdahl, Susan A. ZumdahlPublisher:Cengage Learning
![Text book image](https://www.bartleby.com/isbn_cover_images/9781337399074/9781337399074_smallCoverImage.gif)
![Text book image](https://www.bartleby.com/isbn_cover_images/9781133949640/9781133949640_smallCoverImage.gif)
![Text book image](https://www.bartleby.com/isbn_cover_images/9780534420123/9780534420123_smallCoverImage.gif)
![Text book image](https://www.bartleby.com/isbn_cover_images/9781337398909/9781337398909_smallCoverImage.gif)
![Text book image](https://www.bartleby.com/isbn_cover_images/9781305079243/9781305079243_smallCoverImage.gif)