ideal gas law. ideal gas imaginary gas that conforms to all of the assumptions of the kinetic...
TRANSCRIPT
![Page 1: Ideal Gas Law. Ideal Gas Imaginary gas that conforms to all of the assumptions of the kinetic molecular theory (Day 1)](https://reader036.vdocument.in/reader036/viewer/2022082818/56649e755503460f94b7635d/html5/thumbnails/1.jpg)
Ideal Gas Law
![Page 2: Ideal Gas Law. Ideal Gas Imaginary gas that conforms to all of the assumptions of the kinetic molecular theory (Day 1)](https://reader036.vdocument.in/reader036/viewer/2022082818/56649e755503460f94b7635d/html5/thumbnails/2.jpg)
Ideal Gas
Imaginary gas that conforms to all of the assumptions of the kinetic molecular theory (Day 1)
![Page 3: Ideal Gas Law. Ideal Gas Imaginary gas that conforms to all of the assumptions of the kinetic molecular theory (Day 1)](https://reader036.vdocument.in/reader036/viewer/2022082818/56649e755503460f94b7635d/html5/thumbnails/3.jpg)
Real Gas
Can sometimes conform to all of the assumptions of the kinetic theory it can behave ideally
Does not behave ideally at high pressures and/or low temperatures
![Page 4: Ideal Gas Law. Ideal Gas Imaginary gas that conforms to all of the assumptions of the kinetic molecular theory (Day 1)](https://reader036.vdocument.in/reader036/viewer/2022082818/56649e755503460f94b7635d/html5/thumbnails/4.jpg)
Ideal Gas Law
P = pressureV = Volume (L) n = number of moles R = ideal gas constantT = temperature (K)
P V = n R T
![Page 5: Ideal Gas Law. Ideal Gas Imaginary gas that conforms to all of the assumptions of the kinetic molecular theory (Day 1)](https://reader036.vdocument.in/reader036/viewer/2022082818/56649e755503460f94b7635d/html5/thumbnails/5.jpg)
R: Ideal Gas Constant
R = 0.0821 L atm K mol
R = 62.4 L mmHg K mol
Choose R so that the pressure units match the pressure units in the
problem.
![Page 6: Ideal Gas Law. Ideal Gas Imaginary gas that conforms to all of the assumptions of the kinetic molecular theory (Day 1)](https://reader036.vdocument.in/reader036/viewer/2022082818/56649e755503460f94b7635d/html5/thumbnails/6.jpg)
Example #1:
What is the pressure (in mm Hg) exerted by 85.5 g of CO2 at 27˚C if the gas is contained in a 15.0 L container?
P = ?
V = 15.0 L
n = ? (85.5 g)
R = 62.4 62.4 L mm HgL mm Hg
K molK mol
T = 27oC + 273 = 300 K
![Page 7: Ideal Gas Law. Ideal Gas Imaginary gas that conforms to all of the assumptions of the kinetic molecular theory (Day 1)](https://reader036.vdocument.in/reader036/viewer/2022082818/56649e755503460f94b7635d/html5/thumbnails/7.jpg)
Example #1:
PV = nRTP = nRT
V
![Page 8: Ideal Gas Law. Ideal Gas Imaginary gas that conforms to all of the assumptions of the kinetic molecular theory (Day 1)](https://reader036.vdocument.in/reader036/viewer/2022082818/56649e755503460f94b7635d/html5/thumbnails/8.jpg)
Example #2:What is the mass of 120 L of SO2 at a
temperature of 40˚C and a pressure of 1.85 atm?
P = 1.85 atm
V = 120 L
n = ??? (but want grams)
R = 0.0821 L atm
K mol
T = 40oC + 273 = 313 K
![Page 9: Ideal Gas Law. Ideal Gas Imaginary gas that conforms to all of the assumptions of the kinetic molecular theory (Day 1)](https://reader036.vdocument.in/reader036/viewer/2022082818/56649e755503460f94b7635d/html5/thumbnails/9.jpg)
Example #2:
PV = nRT
n = PVRT
![Page 10: Ideal Gas Law. Ideal Gas Imaginary gas that conforms to all of the assumptions of the kinetic molecular theory (Day 1)](https://reader036.vdocument.in/reader036/viewer/2022082818/56649e755503460f94b7635d/html5/thumbnails/10.jpg)
We can also derive many formulas from PV=nRT to determine other values…Molar Mass = DRT
PMolar Mass = # grams
# moles (n)
Density = P*Molar Mass
RT
![Page 11: Ideal Gas Law. Ideal Gas Imaginary gas that conforms to all of the assumptions of the kinetic molecular theory (Day 1)](https://reader036.vdocument.in/reader036/viewer/2022082818/56649e755503460f94b7635d/html5/thumbnails/11.jpg)
Example 3What is the molar mass of a gas if 0.628g of the gas occupies a volume or 150 mL at 25˚C and 7456 mm Hg pressure?
![Page 12: Ideal Gas Law. Ideal Gas Imaginary gas that conforms to all of the assumptions of the kinetic molecular theory (Day 1)](https://reader036.vdocument.in/reader036/viewer/2022082818/56649e755503460f94b7635d/html5/thumbnails/12.jpg)
Molar Mass = # g 0.628 g
# mol
Use PV=nRT to find the moles:
n = PV
RT