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### 31 Cards in this Set

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 Why are gases weiord? invisible low density ( 1000 * less dense) diffuse/expansion fill any container they are in volume is meaningless particals 1000 m/s pressure force/ surface area force in gases collisions of particles against you/ container surface area where the container/ you is atmosphere 1 atm typical day at sea level pressure of the atmosphere Kinetic energy gas is made of mostly space therefor it is easily compressed and can miz so readily Gas molecules are always moving so the pressure of a gas is the effect of the molecules hitting the walls of the container No energy is formed of used in the movement of the molecules KE remains thesame if temperature and volume does not change Molecules have no attraction or rpulsion to one another measurements 760 mm HG = 1 atm = 76 cm Hg= 101.3 kPa Boyles law the volume of a sample of gas is inversely proportional to its presure if the temperature remains constant equation for Boyles law PV = K P= pressure V= the volume of the sample K= a constant inverse relationships PV = K inverse V/P = K direct equations to inverse relationships P1 V1 = P2 V2 Charles law at a constant pressure the volume of a gas is directly proportional to its Kelvin temperature absotlute zero - 273 so you must add 273 to the temperature is in Celsius Charles law equation V1 V2 or v --- = --- ---- = K T1 T2 T No name law compares presssure and temperature equation for no name law P1 P2 --- = ---- T1 T2 Combined gas laws P1 V1 = P2 V2 P1 V1 P2 V2 ------ = ------- T1 T2 Gas stoichiometry What is the difference using volume but volumes are meaningless molar volume the size of 1 mole of any gas at STP is 22.4 liters Golden Figure 1 mile gas--6.02*10(23)particals 22.4 liter ------------- 1 GMM STP mass to volume X g gi/ 1 m gi/ X m w/ 22.4 l w -------------------------------- /GMM g gi/X m gi/ 1 m w STP volume to mass X l gi/ 1 m gi/ X m w/ GMM g w ------------------------------- /22.4 l gi/ X m gi/ 1 m w non STp volume to mass balance equation gas laws P1 V1 T1 constant =P2 V2 T2 stoich non STP mass to volume balance equation stoich gas laws P1 V1 T1 constant P2 V2 T2 Another way volume to mass PV= n RT (p* cons) -------- (V)=(X)( 8.31) (T+273) (760) Stoich start in middle Another way mass to volume PV= n RT stoich for moles stop in middle ( P) (X )= (m stoi)(8.31)(T+273) Avogadro's Principle equal volumes of gases at equal conditions contain equal numbers of particles Changing conditions Gas laws P1 V1 T1 P2 V2 T2 before after changing conditions STP given M or V want M or v chemical equations changing conditions non STP same as STP with conditions given changing conditions ideal gas laws 1 gas mentioned conditions given no before and after