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Gas Laws

Gas Laws. Alex Daro, Brian Kuttler, and Max O'Donnell. Properties of Gases. Gases have mass Gases are easy to compress Gases fill to their container Diffusion is when gases move through other gases Gases exert pressure. Kinetic Molecular Theory. Gases consist of small particles

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Gas Laws

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  1. Gas Laws Alex Daro, Brian Kuttler, and Max O'Donnell

  2. Properties of Gases • Gases have mass • Gases are easy to compress • Gases fill to their container • Diffusion is when gases move through other gases • Gases exert pressure

  3. Kinetic Molecular Theory • Gases consist of small particles • Particles must be separated by a large distance • Particles are in constant motion • Pressure results when particles collide with a container's wall • Kinetic energy of the gas depends on the temperature of the gas

  4. Temperature's Effect • An increase in temperature will make gas particles move faster • An increase of temperature also makes gas particles spread apart (Increase in volume)

  5. Pressure's Effect • An increase in pressure decreases volume and compresses particles • The particles also become less dense and spread out

  6. Volume's Effect • A decrease in volume results in greater pressure which makes the particles move closer together • As volume increases temperature increases

  7. Pressure Units • atm • torr (mm Hg) • Pa • kPa 1 atm = 760 torr = 101,325 Pa = 101.3 kPa • All answers involving pressure must be in atm unless stated otherwise

  8. Boyle's Law • P1V1 = P2V2 • This states that pressure and volume have an inverse relationship • (780 torrs)(2 Liters) = (? P)(5 Liters) • (78/76 atm)(2 Liters) • 2.05 = ?P(5 Liters) • 2.05(atms * Liters)/(5 liters) • .41 atm = ?P

  9. Charles' Law • V1/T1 = V2/T2 • This states that volume and temperature have a direct relationship • (300mL N)/(30°C) = (?V)(90°C) • (10 mL/°C) = (?V)(90°C) • (.1mL) = (?V)

  10. Gay-Lussac's Law • P1/T1 = P2/T2 • This states that pressure and temperature have a direct relationship • (760mmHg)/(200K) = (?P)(300K) • (3.8 mmHg/K) = (?P)(300K) • (.01 mmHg) = (?P) • (.00002 atm) = (?P)

  11. Combined Gas Law • P1V1/T1 = P2V2/T2 • This is a combination of other gas laws • (2atm)(3.2 L)/?T = (4.5atm)(5 L)/(200K) • 6.4atm*L/?T=.1125atm*L/K • 6.4atm*L=.1125atm*L/K(?T) • ?T = 60 K

  12. Ideal Gas Law • PV = nRT • R = .0821L*atm/(mol*K) • n = Number of moles • P = Pressure • V = Volume • T = Temperature

  13. Ideal Gas Law Problem • 2atm(5) = 3moles*R*?T • 10 atm*L = .2463 ?T • 40 K = ?T

  14. Dalton's Law of Partial Pressure • Each gas and a mixture of gas has its own pressure and the total pressure of the mixture is the sum of the partial pressures of the component gases • PT=P1+P2+P3+...

  15. Practice Problem • If the total pressure of the gas is 1atm and the pressure of hydrogen gas is .2atm then what is the pressure of the nitrogen gas? • 1atm=.2atm+P2 • .8atm = P2

  16. Graham's Law of Effusion • Rates of effusion of gases at the same temperature and pressure are inversely proportional to the square roots of their molar masses • (rate of effusion of A)/(rate of effusion of B) = (root MB)/(root MA) • The rates are found in grams/mole

  17. Practice Problem • What is the rate of effusion of oxygen(O2) and hydrogen(H2)? • √(32 grams/mol)/√(2.016 grams/mol) • Hydrogen effuses 3.98 times faster than oxygen

  18. Graham's Law of Diffusion • Diffusion is the rate at which particles move away from the initial point in space.

  19. Boyles Law Practice Problems #1 5atm(2 Liters) = 4atm(xliters) • 10atm*L/4atm = xliters • x = 2.5 Liters #2 920torr(5 Liters) = xatm(2 Liters) • 1.2atm(5 Liters) = xatm(2 Liters) • 1.2atm*5Liters/2 Liters = x atm • x atm = 3 atm

  20. Charles Law Practice Problems #1 5atm/100K = 10atm/xK • 1atm/20K(xK) = 10 atm • xK = 10atm/(1atm/20K) • xK = 200 K #2 15atm/10K = xatm/200K • 15atm/10k(200K) = xatm • xatm = 300 K

  21. Gay-Lussac's Law Practice Problems #1 5Liters/ 20K = 21Liters/ xK • 1Liter/4K (xK)= 21 Liters • xK = 21Liters/(1liter/4K) • xK = 84K #2 .6Liters/50K = xLiters/21K • .6Liters/50K*21K = xLiters • xLiters = .252 Liters

  22. Combined Gas Law Practice Problems 1.(3atm)(2.2 L)/?T = (4.5atm)(6 L)/(200K) (6.6atm*L)/(?T)=(.135atm*L/K) (48.89K)=(?T) 2. (?atm)(4.3 L)/200K = (3atm)(3 L)/(273K) (?atm)(4.3L)/200K = (.03atm*L/K) (?atm)(4.3L) = (6atm*L) (?atm) = (1.4atm)

  23. Ideal Gas Law Practice Problems 1. 1atm(3L)=?n*R*273K (3atm*L)=(?n)(22.4L*atm/(mol)) (.13moles)=(?n) 2. ?atm(4L)=3*R*273K ?atm(4L)=67.24L*atm/(mol) ?atm=16.84atm

  24. Dalton's Law of Partial Pressures Practice Problems 1) If the pressure of Hydrogen gas is .35 atm and Nitrogen gas is .47 atm and Oxygen gas is .24 atm what is the total pressure? .35 + .47 + .24 = PT PT = 1.06

  25. Dalton's Law of Partial Pressures Practice Problems Cont. 2) If the total pressure of gases is 3.01 atm then what is the pressure of Oxygen gas if the pressure of Hydrogen gas is 1.11 atm and the pressure of Nitrogen gas is .87 atm? 3.01 atm = P1 atm + 1.11 atm + .87 atm 3.01 atm = P1 atm + 1.98 atm P1 atm = 1.03 atm

  26. Graham's Law of Effusion 1) What is the rate of effusion of Oxygen gas (O2) and Nitrogen gas (N2)? √(32 grams/mol)/√(28.02 grams/mol) Nitrogen effuses 1.069 times faster than oxygen

  27. Graham's Law of Effusion Cont. 2) What is the rate of effusion of Nitrogen gas (N2) and Hydrogen gas (H2)? √(28.02 grams/mol)/√(2.016 grams/mol) Hydrogen effuses 3.728 times faster than oxygen

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