Ideal Gas Law
What is the pressure in atm of 1.00g of NH3(g) in a 500mL container at 20 C?
See attached file for full problem description.
© BrainMass Inc. brainmass.com October 24, 2018, 5:52 pm ad1c9bdddfhttps://brainmass.com/chemistry/organic-chemistry/ideal-gas-law-pressures-23409
Attachments
Solution Preview
Please see the attached file.
Use the ideal gas law PV=nRT to obtain P
You will need to find n - the moles of gas present. Don't forgrt to convert T from celsius to kelvin.
You may want to look at the following sites:
http://scienceworld.wolfram.com/physics/IdealGasLaw.html
http://hyperphysics.phy-astr.gsu.edu/hbase/kinetic/idegas.html#c1
• What is the pressure in atm of 1.00g of NH3(g) in a 500mL container at ...
Solution Summary
A simple example of the ideal gas equation and units conversion.
The Ideal Gas Law to Determine the Molecular Weights of Gas
At a given temperature a certain number of grams of CH4, when placed in a 10 L vessel, exerts a pressure of 0.240 atm. An equal number of grams of gas B, when placed in a 12 L container at the same temperature, exerts a pressure of 0.145 atm. Calculate the approximate molecular weight of gas B.
View Full Posting Details