Interpretation:
The partial pressures of helium and neon are to be calculated with given volume, pressure, and temperature.
Concept Introduction:
The ideal gas equation elaborates the physical properties of gases by relating the pressure, volume, temperature, and number of moles with each other with the help of four
Here,
The expression to calculate mole fraction
Here,
The relation between partial pressure
The conversion of temperature from degree Celsius to Kelvin can be done by using the formula given below:
Answer to Problem 106AP
Solution:
Explanation of Solution
Given information: For
Volume is
Pressure is
Temperature is
For
Volume is
Pressure is
Temperature is
After the stopcock is opened, both the gases mix togethercompletely.
First, find the number of moles of each gas with the help of theideal gas equation as
Temperature is in Celsius. Convert it into Kelvin as
For
Substitute
For
Substitute
Calculate the total number of moles as
Substitute
Now, rearrange theideal gas equation for
Substitute
The formula to calculate the mole fraction is
Now, calculate the mole fractions of each component.
For
Substitute
For
Substitute
The relation between partial pressure and total pressure is
For
Substitute
For
Substitute
The partial pressures of helium and neon are
Want to see more full solutions like this?
Chapter 10 Solutions
Aleks 360 Access Card 1 Semester For Introductory Chemistry
- A 275-mL sample of CO gas is collected over water at 31C and 755 mmHg. If the temperature of the gas collection apparatus rises to 39C, what is the new volume of the sample? Assume that the barometric pressure does not change.arrow_forwardA mixture at 33 °C contains H2at 325 torr. N;at 475 tore and O2at 650. torr. What is the total pressure of the gases in the system? Which gas contains the greatest number of moles?arrow_forwardIn the anaerobic oxidation of glucose by yeast, CO2 is produced: If 1.56 L of CO2 were produced at 22.0 C and 0.965 atm, what mass of C6H12O6 is consumed by the yeast? Assume the ideal gas law applied.arrow_forward
- How would the use of a volatile liquid affect the measurement of a gas using open-ended manometers vs. closed-end manometers?arrow_forwardA sample of a smoke stack emission was collected into a 1.25-L tank at 752 mm Hg and analyzed. The analysis showed 92% CO2, 3.6% NO, 1.2% SO2, and 4.1% H2O by mass. What is the partial pressure exerted by each gas?arrow_forwardHelium gas, He, at 22C and 1.00 atm occupied a vessel whose volume was 2.54 L. What volume would this gas occupy if it were cooled to liquid-nitrogen temperature (197C)?arrow_forward
- Sulfur 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_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
- Chemistry: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher:Cengage LearningChemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage Learning
- Chemistry & Chemical ReactivityChemistryISBN:9781337399074Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage LearningIntroductory Chemistry: A FoundationChemistryISBN:9781285199030Author:Steven S. Zumdahl, Donald J. DeCostePublisher:Cengage LearningChemistry for Engineering StudentsChemistryISBN:9781337398909Author:Lawrence S. Brown, Tom HolmePublisher:Cengage Learning