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THE IDEAL GAS LAW Michael Knowles Andrew Smith Trey Thompson.

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1 THE IDEAL GAS LAW Michael Knowles Andrew Smith Trey Thompson

2 Ideal Gas Law Introduction The ideal gas Law says PV=nRT Pressure*Volume=number of moles of the gas*Universal gas constant*Temperature of the gas The Ideal Gas Law was first stated by Benoît Paul Émile Clapeyron in 1834 as a combination of Boyless and Charless laws, with Avogadros and Gay-Lussacs laws included later The Ideal Gas Law is only applicable when gases behave themselves and conform to gas laws at all pressures and temperatures (ideal gases)

3 Benoît Paul Émile Clapeyron Benoît Clapeyron was born on February 26, 1799 in Paris, France and lived in both France and Russia. Beyond the Ideal Gas Law, Clapeyron was also a founder of thermodynamics, another branch of natural science. He supervised the construction of the first railway to connect Paris, Versailles, and Saint- Germain. He was married to Mélanie Bazaine. He died in Paris on January 28, 1864.

4 Ideal Gas Law in Everyday Life: Air Conditioners The refrigeration and heating cycles found in air conditioners take advantage of the Ideal Gas Law by altering pressures to change the temperature of the gas released. Compressing gasses gives off energy as heat. Decompressing gasses absorbs heat. Air conditioners do this in a constant loop. Inside your house, a gas is depressurized, absorbing heat from the room in the process, cooling the air. The low pressure gas is then pumped outside. Outside, the gas is compressed, releasing the heat energy taken from inside. Then it heads back in. Over and over again. 1) condensing coil, 2) expansion valve, 3) evaporator coil, 4) compressor. pump.svg

5 Real World Visual Procedure: Stretch the balloon over the opening of the Erlenmeyer Flask. Heat up the air inside of the flask using a hot plate. Observe. AAAAAABps/4aY_Qw- hqK8/s400/MatterGas2010+004.jpg

6 Problem Worked Out 2.50 g of XeF 4 gas is placed into an evacuated 3.00 liter container at 80°C. What is the pressure in the container? PV = nRT, where P is pressure, V is volume, n is number of moles, R is the gas constant, and T is temperature. P=? V = 3.00 liters n = 2.50 g XeF4 x 1 mol/ 207.3 g XeF4 = 0.0121 mol R = 0.0821 l·atm/(mol·K) T = 273 + 80 = 353 K Plugging in the values: P = nRT/V P = 00121 mol x 0.0821 l·atm/(mol·K) x 353 K / 3.00 liter P = 0.117 atm Answer: 0.117 atm

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