Log in
Chemistry
2
answers
0
watching
17
views
23 Nov 2019

The composition of dry air at sea level is 78.03% N2, 20.99% O2, and 0.033% CO2 by volume. (a) calculate the average molar mass of this air sample (b) calculate the partial pressures of N2, O2, and CO2 in atm. (at constant temperature and pressure, the volume of a gas is directly proportional to the number of moles of the gas). Also what should be used for constant temperature and pressure?

Watch
2
answers
0
watching
17
views

For unlimited access to Homework Help, a Homework+ subscription is required.

Unlock all answers

Get 1 free homework help answer.
Get unlimited access
Already have an account? Log in
Share
Trinidad Tremblay
Trinidad TremblayLv2
12 Jan 2019
Get unlimited access
Already have an account? Log in
Share
discord banner image
Join us on Discord
Chemistry Study Group
Join now

Related textbook solutions

Basic Chemistry
5 Edition,
Timberlake
ISBN: 9780134138046
Principles of Chemistry Molecular Approach
4th Edition,
Tro
ISBN: 9780134112831
Chemistry: Structure and Properties
2nd Edition,
Tro
ISBN: 9780134293936
Principles of Chemistry Molecular Approach
3rd Edition, 2014
Tro
ISBN: 9780321971944
Chemistry: A Molecular Approach
3rd Edition,
Tro
ISBN: 9780321809247
Chemistry: A Molecular Approach
5th Edition,
Tro
ISBN: 9780134874371
Principles of Chemistry: A Molecular Approach
4th Edition,
Tro
ISBN: 9780134895741
Chemistry: The Central Science
14th Edition, 2017
Brown
ISBN: 9780134414232

Related questions

The composition of dry air at sea level is 78.03% N2,20.99% O2, and 0.033% CO2 by volume.

a.)Calculate the average molar mass of this air sample.

b.) Calculatethe partial pressures of N2, O2, andCO2 in atm.

(At constant temperature and pressure, thevolume of a gas is directly proportional to the number of moles ofthe gas.)

A sample of air is collected over water at 50.00°C. At equilibrium, the total pressure of the moist air is 1.0100 atm. The equilibrium vapor pressure of water at 50.00 °C is 92.5876 mmHg. The composition of dry air is 80.00 mol% N2, 19.00 mol% O2, and 1.000 mol% Ar. a) Calculate the partial pressures in atm of N2, O2, and Ar in the wet mixture assuming ideal gas behavior. b) Calculate the mole fractions of H2O, N2, O2, and Ar in the wet mixture, again assuming ideal gas behavior. c) Calculate the mass fractions of H2O, N2, O2, and Ar in the wet mixture, again assuming ideal gas behavior. d) Calculate the average molecular weight of the wet and dry air in units of g/mol.

Dry air near sea level has the following composition by volume: N2,78.08 percent; O2, 20.94 percent; Ar, 0.93 percent; CO2, 0.05percent. The atmospheric pressure is 1.00 atm. (Hint: Since volumeis proportional to the number of moles present, mole fractions ofgases can be expressed as ratios of volumes at the same temperatureand pressure.)
Calculate the concentration of each gas in moles per liter at 0°C.

Weekly leaderboard

Home
Homework Help 3,900,000
Chemistry 830,000
Start filling in the gaps now
Log in