Concept explainers
Determine the mole fraction of helium in a gaseous mixture consisting of 0.524 g He, 0.275 g Ar, and 2.05 g CH4.
(a) 0.0069
(b) 0.0259
(c) 0.481
(d) 0.493
(e) 0.131
Interpretation:
The mole fraction of Helium in a gaseous mixture has to be calculated.
Concept introduction:
The mole fraction is calculated using below the formula
Answer to Problem 11.1KSP
The mole fraction of Helium in a gaseous mixture is
Explanation of Solution
To determine: The mole fraction of Helium in a gaseous mixture
Reasons for correct options:
The mole fraction of Helium in a gaseous mixture is calculated below
Given,
Where
The mole fraction of Helium in a gaseous mixture is
So the correct answer is option (d)
Reasons for incorrect options:
The calculated result shows that the mole fraction of Helium in a gaseous mixture is
The mole fraction of Helium in a gaseous mixture was calculated.
Want to see more full solutions like this?
Chapter 11 Solutions
Chemistry: Atoms First
- perform stoichiometric ca1cu1uions for reactions involving gases as reactants or products.arrow_forwardHow does hydraulic fracturing differ from previously used techniques for the recovery of natural gas from the earth?arrow_forwardGiven 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_forward
- Liquid oxygen was first prepared by heating potassium chlorate, KClO3, in a closed vessel to obtain oxygen at high pressure. The oxygen was cooled until it liquefied. 2KClO3(s)2KCl(s)+3O2(g) If 171 g of potassium chlorate reacts in a 2.70-L vessel, which was initially evacuated, what pressure of oxygen will be attained when the temperature is finally cooled to 25C? Use the preceding chemical equation and ignore the volume of solid product.arrow_forwardIf the rms speed of He atoms in the exosphere (highest region of the atmosphere) is 3.53 103 m/s, what is the temperature (in kelvins)?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_forward
- Chemistry: Matter and ChangeChemistryISBN:9780078746376Author:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl WistromPublisher:Glencoe/McGraw-Hill School Pub CoIntroductory Chemistry: A FoundationChemistryISBN:9781337399425Author:Steven S. Zumdahl, Donald J. DeCostePublisher:Cengage LearningLiving By Chemistry: First Edition TextbookChemistryISBN:9781559539418Author:Angelica StacyPublisher:MAC HIGHER
- Chemistry for Engineering StudentsChemistryISBN:9781337398909Author:Lawrence S. Brown, Tom HolmePublisher:Cengage LearningIntroductory Chemistry: An Active Learning Approa...ChemistryISBN:9781305079250Author:Mark S. Cracolice, Ed PetersPublisher:Cengage LearningWorld of Chemistry, 3rd editionChemistryISBN:9781133109655Author:Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCostePublisher:Brooks / Cole / Cengage Learning