The Ideal Gas Law
Lecture 2 How to measure pressure of a gas? Simple barometer
The pressure of air pushing down is vacuum strong enough to support a column of mercury that is 76 cm high. This (no air) defines the “standard atmosphere”.
force Mg P = = area A Mass M ρ ρV g ρAh g Density = = = ρhg (13.6 x 103 kg/m3 ) A A 1 Stnd. Atm. = 1.013 x 105 Pa Area of ≈ 100 kPa = 0.1 MPa tube A = 14.7 psi = 760 torr (1 Pa = 1 N/m2) How does P and V of gas vacuum depend on T? (no air)
P= ρgh
V (volume)
T (liquid bath); externally controlled P-V Data for Low Pressure Gas
T must be measured in Kelvins! Analysis of Data Shows
PV = Constant T
Ideal Gas Law Constant Careful experiments on low density gasses show
PV = constant = k N T N = number of molecules
PV = N k T k = Boltzman’s Constant = 1.381 x 10-23 J/K = 8.617 x 10-5 eV/K Units?
Physics Chemistry P in Pascal P in Pascal V in m3 V in liters T in Kelvin T in Kelvin N is number of molecules n is molar fraction PV = NkT PV = nRT
10 cm 1 liter = 1000 cm3 10 cm 1 mole is number of atoms = 0.001 m3 in 12 grams of carbon-12 10 cm Moles!
Avagadro’s hypothesis: Equal volumes of different gasses at same pressure and temperature contain
the same number of molecules (NA). NA is NOT a fundamental physical constant; it’s a conversion factor between microscopic mass units (amu) and macroscopic mass units (grams).
1 gm = NA x 1 amu
1 amu = 1.6605 x 10-27 kg
23 NA ≅ 6.023 x 10 Moles, Avagadro’s Number and the Universal Gas Constant R
Since PV=NkT=nRT and defining the
molar fraction n = N/NA
6.02 x 1023 1.381 x 10-23 J 8.314 J R = N k = x = A mole K mole K 8.314 J 1 Nm 1m2 = x x mole K J 1m2 8.314 N m3 1 liter 1 atm = x x m2 mole K 0.001 m3 1.013 x 105 N/m2 liter atm = 0.08206 mole K A Universal Law? The Ideal Gas Law
Expect horizontal straight line Examples
1. What is the volume of 1 mole of gas at STP?
Note:
STP: 0oC (273.15 K), 1 atm (101.325 kPa) SNP: 20oC (293.15 K), 1 atm (101.325 kPa) 2. The best vacuum that can be obtained in a laboratory is about 1 x 10-13 Pa. How many molecules per cc at 273 K? 3. Fill a balloon with helium gas to a radius of 18 cm. The temperature of balloon is 20 C. The pressure inside is 1.05 atm. How many moles of helium gas are required? 4. A storage tank of compressed helium has a volume of 30 liters and a pressure of 30 atm at 20oC. How many balloons will the tank fill? 5. If you fill a 500 liter storage container with 25.5 moles of gas at 10C, what is the gauge pressure of the gas in the tank? Beyond the Ideal Gas Law
1. van der Waals equation (empirical): {P + a(n/V)2 } {V/n – b} = RT
P increased by long V reduced by finite range attraction size of molecules
2. Virial expansion:
B(T) is first virial coefficient, C(T) is second virial coefficient, etc.
Note: Virial is derived from the Latin word for “force”. Virial is a word commonly used to describe a function related to force.