The Gas Laws -_________ ________ provides a ______ that explains the properties of ________, _________, and ______ in terms of __________ that are always in ________ and the ________ that exist between them kinetictheorymodel solidsliquids I. Kinetic Theory gasesparticles motionforces -actual gases don’t always obey, but ___________ the ____________made by the _________ ________ approximate assumptionskinetic theory A. Gas particles do not attract or repel eachother B. Gas particles are much smaller than the distances between them C. Gas particles are in constant, random motion D. No energy is lost in the collisions of gas particles E. All gases have same average kinetic energy at same temperature

The Gas Laws II. Boyle’s Law-the _______ of a gas _________ _________ with the _________, providing the ___________ is held ________ Robert Boyle ( ) volumevariesinversely pressuretemperature constant P1V1P1V1 =P2V2P2V2 or P1P1 P2P2 ___ = V2V2 V1V1 If a sample of Argon gas occupies a volume of 10.0 liters at a pressure of 200 kilopascals, at what pressure would the same sample of gas occupy 5.0 liters, if the temperature remains constant? P1P1 P2P2 ___ = V2V2 V1V1 200 kPa P2P2 ______ = 5.0 L 10.0 L ____ P2P2 =400 kPa

The Gas Laws II. Boyle’s Law Boyle’s Vacuum Chamber, Designed by Robert Hooke If a sample of Carbon dioxide gas occupies a volume of 35.0 liters at a pressure of 1.10 atmospheres, what volume would the same sample of gas occupy at 1.25 atmospheres, if the temperature remains constant? P1P1 P2P2 ___ = V2V2 V1V atm 1.25 atm _______ = V2V L _____ V2V2 =30.8 L

The Gas Laws III. Charles’s Law-the _______ of a gas _________ _________ with the ___________, providing the _________ is held ________ Jacques Charles ( ) volumevariesdirectly temperaturepressure constant V1T2V1T2 =V2T1V2T1 or V1V1 V2V2 ___ = T1T1 T2T2 If a sample of Chlorine gas occupies a volume of 250 milliliters at a temperature of 22°C, what volume would the same sample of gas occupy at -22°C, if the pressure remains constant? V1V1 V2V2 ___ = T1T1 T2T2 250 mL V2V2 ______ = 22°C -22°C ____ V2V2 =-250 mL? A negative volume? We need a temperature scale with no zero, and no negative values! K= °C mL V2V2 ______ = 295 K 251 K _____ V2V2 =213 mL

The Gas Laws III. Charles’s Law-_________ _____ is the _______ possible theoretical temperature, equal to _________, and is the ___________ at which the ________ of a sample of gas is _____, and all ________, __________ movement of particles ________ absolutezerolowest °C volumetemperature zerorandom Brownianceases -the coldest _______ temperature is _______, or _________, the temperature of ______ _______ actual4.22 K °CliquidHelium William Thomson (Lord Kelvin) ( )

The Gas Laws III. Charles’s Law If a sample of methane gas occupies a volume of liters at a temperature of 68°F, at what temperature, in °F, would the same sample of gas occupy liters, if the pressure remains constant? V1V1 V2V2 ___ = T1T1 T2T L L ______ = 293 K T2T2 _____ T2T2 =318 K °F +9/5 Charles’s Hydrogen-filled balloon over Paris, 1783 K= °C +273 =°C32 T2T2 =113°F

The Gas Laws IV. Gay-Lussac’s Law-the _______ of a gas _________ _________ with the ___________, providing the _________ is held ________ Joseph Gay-Lussac ( ) pressurevariesdirectly temperature volume constant P1T2P1T2 =P2T1P2T1 or P1P1 P2P2 ___ = T1T1 T2T2 If the pressure in a propane tank is 965 mm Hg at a temperature of 25°C, what would the pressure in the tank be at 50°C, if the volume remains constant? P1P1 P2P2 ___ = T1T1 T2T2 K= °C mm Hg P2P2 _________ = 298 K 323 K _____ P2P2 =1040 mm Hg

The Gas Laws IV. Gay-Lussac’s Law If the air pressure in an autoclave is 833 torr at a temperature of 212°F, at what temperature, in °F, would the air pressure be 900 torr, if the volume remains constant? P1P1 P2P2 ___ = T1T1 T2T2 833 torr 900 torr ______ = 373 K T2T2 _____ T2T2 =403 K °F +9/5 Gay-Lussac and Jean-Baptiste Biot in Hydrogen balloon, 1804 K=°C+273 =°C32 T2T2 =266°F

The Gas Laws V. Combined Gas Law-the _______ of a gas is _________ proportional to ________ and directly proportional to ___________, and ________ is __________ proportional to ____________ pressureinversely volume directly temperature volume P1V1P1V1 = P2V2P2V2 _____ T1T1 T2T2 If the volume of a sample of Hydrogen sulfide gas is 2.00 liters at a pressure of 110 kilopascals and a temperature of 30.0°C, what is the volume of the same sample of Hydrogen sulfide, in liters, at a temperature of 80.0°C and a pressure of 440 kilopascals? K= °C +273 (2.00 L) K _____________ = K (440 kPa) __________ V2V2 =0.582 L temperature P1V1P1V1 = P2V2P2V2 _____ T1T1 T2T2 (110 kPa)V2V2

The Gas Laws V. Combined Gas Law If a Helium-filled balloon at sea level has a volume of 2.1 liters at a pressure of atmospheres and a temperature of 36°C, and it is released and rises to an elevation at which the temperature is 28°C and the pressure is atmospheres, what will be the new volume of the balloon? K= °C +273 (2.1 L) 309 K _____________ = 301 K (0.900 atm) __________ V2V2 =2.3 L P1V1P1V1 = P2V2P2V2 _____ T1T1 T2T2 (0.998 atm) V2V2

The Gas Laws VI. Avogadro’s Principle-______ ________ of gases at the same ____________ and _________ contain ______ numbers of ________ equalvolumes temperature particles pressure equal mole -one ______ of gas contains __________ particles and occupies _______ at _________ temperature and pressure, which is ______ and ________ 6.02 x L standard 0.00°C1.00 atm Amadeo Avogadro ( ) How many molecules in 3.73 liters of ozone at STP? 3.73 L O 3 x 1 mole O 3 ___________ 22.4 L O 3 =1.00 x molecules O 3 conversion factor x 6.02 x molecules O 3 _________________ 1 mole O 3

The Gas Laws VI. Avogadro’s Principle What is the volume, in liters, of moles of Fluorine gas at STP? mole F 2 x 22.4 L F 2 ________ 1 mole F 2 =19.7 L F 2 How many moles of Nitrogen gas are in 2.00 liters at STP? 2.00 L N 2 x 1 mole N 2 ________ 22.4 L N 2 = moles N 2 What is the volume, in liters, of 5.0 kilograms of methane at STP? 5.0 kg CH 4 x 1000 grams CH 4 ____________ 1 kg CH 4 =7.0 x 10 3 L CH 4 conversion factor x 1 mole CH 4 ______________ grams CH 4 x 22.4 L CH 4 _________ 1 mole CH 4 What mass, in grams, of Nitrogen dioxide occupies liters at STP? L NO 2 x 1 mole NO 2 __________ 22.4 L NO 2 =31.8 g NO 2 x grams NO 2 ______________ 1 mole NO 2