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Published byAnnabel Creed Modified over 2 years ago

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Charles Law V 1 = V 2 P constant T 1 T 2 T 1 T 2 Boyles Law P 1 V 1 = P 2 V 2 T constant Combined P 1 V 1 = P 2 V 2 T 1 T 2 T 1 T 2 Gay-Lussacs Law P 1 = P 2 V constant T 1 T 2 T 1 T 2 ALL temperatures must be in Kelvin!!

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Ideal Gas Equation PV=nRT P pressure V volume (L) n moles T temperature (K) R gas constant 62.4 Ltorr molK.082 Latm molK 8.31 LkPa molK

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Find Volume What volume would be occupied by 1.00 moles of gas at 0˚C and 1 atm pressure? V= nRT=(1.00 mole)(.082 Latm/molK)(273K) P 1 atm P 1 atm = 22.4L = 22.4L

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When given three of the four variables, we can find the fourth. A gas has a volume of 2.20L at 25 C. If there are.085 moles of the gas, under what pressure must the gas be held? A gas has a volume of 2.20L at 25 C. If there are.085 moles of the gas, under what pressure must the gas be held? P = nRT P = nRT V P = (.085mole)( Latm)(298K) P = (.085mole)( Latm)(298K) 2.20L molK 2.20L molK =.945 atm (or 95.8 kPa or 718 torr) =.945 atm (or 95.8 kPa or 718 torr)

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Find moles A gas has a volume of 31.2L at 28˚C and 82.6 kPa. How many moles are in the sample? n = PV = (82.6kPa)(31.2L) RT (8.31kPaL/molK)(301K) RT (8.31kPaL/molK)(301K) = 1.03 mol = 1.03 mol How many molecules would that be? 1.03 mol x 6.02 x molecules/mol = 6.20 x molecules = 6.20 x molecules

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