Lecture 4 Ideal Gas Law and Kinetic Theory
Today s Topics: Ideal Gas Law Kinetic Theory of Gases Phase equilibria and phase diagrams
Ideal Gas Law An ideal gas is an idealized model for real gases that have sufficiently low densities. The condition of low density means that the molecules are so far apart that they do not interact except during collisions, which are effectively elastic. At constant volume the pressure is proportional to the temperature. P µ T
At constant temperature, the pressure is inversely proportional to the volume. P µ 1 V n The pressure is also proportional to the amount of gas. P µ n number of moles of gas
Moles and Avogadro s Number One mole of a substance contains as many particles as there are atoms in 1 grams of the isotope carbon-1. The number of atoms per mole is known as Avogadro s number, N A. N A 6.0 10 3 mol -1 n N N A number of moles number of atoms
The mass per mole (in g/mol) of a substance has the same numerical value as the atomic or molecular mass of the substance (in atomic mass units). For example, hydrogen has an atomic mass of 1.00794 g/mol, while the mass of a single hydrogen atom is 1.00794 u. Mass of sample n m m particle particle N N A Mass m per mole Mass per mole
The absolute pressure of an ideal gas is directly proportional to the Kelvin temperature and the number of moles of the gas and is inversely proportional to the volume of the gas. P nrt V n N N A R ( mol K) 8. 31J k R N A.31J 6.0 10 ( mol K) 8-3 3 1.38 10-1 mol J K
Consider a sample of an ideal gas that is taken from an initial to a final state, with the amount of the gas remaining constant. PV nrt PV T nr constant P V f T f f PV i T i i Constant T, constant n: P V PV Boyle s law f f i i Constant P, constant n: V f V i Charles law T f T i
Example A sample of a monatomic ideal gas is originally at 0 C. What is the final temperature of the gas if both the pressure and volume are doubled? PV nrt PV T const
Example A sealed container has a volume of 0.00 m 3 and contains 15.0 g of molecular nitrogen (N ) which has a molecular mass of 8.0 u. The gas is at a temperature of 55 K. What is the absolute pressure of the nitrogen gas? PV P nrt nrt V 15g n 0. 536mol 8g / mol
Kinetic Theory of Gases The particles are in constant, random motion, colliding with each other and with the walls of the container. Each collision changes the particle s speed. As a result, the atoms and molecules have different speeds.
THE DISTRIBUTION OF MOLECULAR SPEEDS v rms 970 m/s
Ideal Gases: Pressure, Temperature and Kinetic Energy The origin of pressure: å F x ma x m Dv Dt x D ( mv ) Dt x Average force Final momentum- Initial momentum Time between successivecollisions (- mv )- ( + mv ) x L v x x - mv L x
L mv F x For our single molecule, the average force on the wall is: For N molecules in 3D, the average force is: ø ö ç ç è æ ø ö ç è æ L mv N F 3 mean-square speed ø ö ç ç è æ ø ö ç è æ 3 3 L mv N L F A F P volume ø ö ç ç è æ ø ö ç è æ V mv N P 3 ( ) ( ) 1 3 3 1 rms mv rms N mv N PV NkT KE
THE INTERNAL ENERGY OF A MONATOMIC IDEAL GAS Average translational kinetic energy per particle: 1 mv 3 rms KE kt 3 U N kt 3 nrt Internal energy of an ideal gas
Example Assume that N behaves as an ideal gas and determine the rms speed of the nitrogen molecules when the temperature of the air is 93K. 1 3 mv rms kt m Mass per mol ( g / mol) -1 N ( mol ) A For nitrogen 3kT v rms m m 8.0g mol -3-4.65 10 g 4.65 10 3-1 6.0 10 mol 6 kg
Phase Equilibrium If a liquid is put into a sealed container so that there is a vacuum above it, some of the molecules in the liquid will vaporize. Once a sufficient number have done so, some will begin to condense back into the liquid. Equilibrium is reached when the numbers remain constant.
The pressure of the gas when it is in equilibrium with the liquid is called the equilibrium vapor pressure, and will depend on the temperature. The vaporization curve determines the boiling point of a liquid: A liquid boils at the temperature at which its vapor pressure equals the external pressure.
This curve can be expanded. When the liquid reaches the critical point, there is no longer a distinction between liquid and gas; there is only a fluid phase. The fusion curve is the boundary between the solid and liquid phases; along that curve they exist in equilibrium with each other. The sublimation curve marks the boundary between the solid and gas phases. The triple point is where all three phases are in equilibrium.
The wonder of sweat! A liquid in a closed container will come to equilibrium with its vapor. However, an open liquid will not, as its vapor keeps escaping it will continue to vaporize without reaching equilibrium. As the molecules that escape from the liquid are the higher-energy ones, this has the effect of cooling the liquid. This is why sweating cools us off.