Presentation on theme: "Not so long ago, in a chemistry lab far far away… May the FORCE/area be with you."— Presentation transcript:
Not so long ago, in a chemistry lab far far away… May the FORCE/area be with you
Ideal Gases Ideal gases are imaginary gases that perfectly fit all of the assumptions of the kinetic molecular theory: 1)Gases consist of tiny particles that are far apart relative to their size. Volume of particles assumed to be negligible. 2) Collisions between gas particles and between particles and the walls of the container are elastic collisions. Assume particles are in constant motion. 3) There are no forces of attraction between gas particles 4) The average kinetic energy of gas particles depends on temperature, not on the identity of the particle.
The Nature of Gases Gases expand to fill their containers Gases are fluid – they flow Gases have low density 1/1000 the density of the equivalent liquid or solid Gases are compressible Gases effuse and diffuse
Pressure Is caused by the collisions of molecules with the walls of a container is equal to force/unit area SI units = Newton/meter 2 = 1 Pascal (Pa) 1 atmosphere = 101,325 Pa 1 atmosphere = 1 atm = 760 mm Hg = 760 torr 1 atm = 29.92inHg = 14.7 psi = bar = 10 m column of water.
Measuring Pressure The first device for measuring atmospheric pressure was developed by Evangelista Torricelli during the 17 th century. The device was called a barometer Baro = weight Meter = measure
An Early Barometer The normal pressure due to the atmosphere at sea level can support a column of mercury that is 760 mm high.
Standard Temperature and Pressure STP P = 1 atmosphere, 760 torr T = C, 273 Kelvins The molar volume of an ideal gas is liters at STP
Converting Celsius to Kelvin Gas law problems involving temperature require that the temperature be in KELVINS! Kelvins = C °C = Kelvins - 273
The Combined Gas Law The combined gas law expresses the relationship between pressure, volume and temperature of a fixed amount of gas. Boyles law, Gay-Lussacs law, and Charles law are all derived from this by holding a variable constant.
Boyles Law Pressure is inversely proportional to volume when temperature is held constant.
Charless Law The volume of a gas is directly proportional to temperature, and extrapolates to zero at zero Kelvin. (P = constant)
Gay Lussacs Law The pressure and temperature of a gas are directly related, provided that the volume remains constant.
Avogadros Law For a gas at constant temperature and pressure, the volume is directly proportional to the number of moles of gas (at low pressures). V = an a = proportionality constant V = volume of the gas n = number of moles of gas
Ideal Gas Law PV = nRT P = pressure in atm V = volume in liters n = moles R = proportionality constant = L atm/ mol· T = temperature in Kelvins Holds closely at P < 1 atm
Standard Molar Volume Equal volumes of all gases at the same temperature and pressure contain the same number of molecules. - Amedeo Avogadro
Gas Density … so at STP…
Density and the Ideal Gas Law Combining the formula for density with the Ideal Gas law, substituting and rearranging algebraically: M = Molar Mass P = Pressure R = Gas Constant T = Temperature in Kelvins
Gas Stoichiometry #1 If reactants and products are at the same conditions of temperature and pressure, then mole ratios of gases are also volume ratios. 3 H 2 (g) + N 2 (g) 2NH 3 (g) 3 moles H mole N 2 2 moles NH 3 3 liters H liter N 2 2 liters NH 3
Gas Stoichiometry #2 How many liters of ammonia can be produced when 12 liters of hydrogen react with an excess of nitrogen in a closed container at constant temperature? 3 H 2 (g) + N 2 (g) 2NH 3 (g) 12 L H 2 L H 2 = L NH 3 L NH
Gas Stoichiometry #3 How many liters of oxygen gas, at STP, can be collected from the complete decomposition of 50.0 grams of potassium chlorate? 2 KClO 3 (s) 2 KCl(s) + 3 O 2 (g) = L O g KClO 3 1 mol KClO g KClO 3 3 mol O 2 2 mol KClO L O 2 1 mol O
Gas Stoichiometry #4 How many liters of oxygen gas, at 37.0 C and atmospheres, can be collected from the complete decomposition of 50.0 grams of potassium chlorate? 2 KClO 3 (s) 2 KCl(s) + 3 O 2 (g) = n mol O g KClO 3 1 mol KClO g KClO 3 3 mol O 2 2 mol KClO 3 = mol O 2 = 16.7 L
Daltons Law of Partial Pressures For a mixture of gases in a container, P Total = P 1 + P 2 + P This is particularly useful in calculating the pressure of gases collected over water.
Diffusion: describes the mixing of gases. The rate of diffusion is the rate of gas mixing. Diffusion
Effusion Effusion: describes the passage of gas into an evacuated chamber.
I look like Abe Lincoln but Im really Thomas Graham!
Effusion: Diffusion: Grahams Law Rates of Effusion and Diffusion
Real Gases corrected pressure corrected volume P ideal V ideal Must correct ideal gas behavior when at high pressure (smaller volume) and low temperature (attractive forces become important).