1 / 59

GASES

GASES. Chapter 5. A Gas. Uniformly fills any container. Mixes completely with any other gas Exerts pressure on its surroundings. Simple barometer invented by Evangelista Torricelli. Pressure. is equal to force/unit area SI units = Newton/meter 2 = 1 Pascal (Pa)

gary-norris
Télécharger la présentation

GASES

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript

  1. GASES Chapter 5

  2. A Gas • Uniformly fills any container. • Mixes completely with any other gas • Exerts pressure on its surroundings.

  3. Simple barometer invented by Evangelista Torricelli

  4. Pressure • is equal to force/unit area • SI units = Newton/meter2 = 1 Pascal (Pa) • 1 standard atmosphere = 101,325 Pa • 1 standard atmosphere = 1 atm = 760 mm Hg = 760 torr

  5. Pressure Unit Conversions • The pressure of a tire is measured to be 28 psi. What would the pressure in atmospheres, torr, and pascals. • (28 psi)(1.000 atm/14.69 psi) = 1.9 atm • (28 psi)(1.000 atm/14.69 psi)(760.0 torr/1.000atm) = 1.4 x 103 torr • (28 psi)(1.000 atm/14.69 psi)(101,325 Pa/1.000 atm) = 1.9 x 105 Pa

  6. Simple Manometer

  7. Volume of a gas decreases as pressure increases at constant temperature

  8. P vs V V vs 1/P BOYLE’S LAW DATA

  9. Boyle’s Law* • (Pressure)( Volume) = Constant (T = constant) • P1V1 = P2V2 (T = constant) • V 1/P (T = constant) • (*Holds precisely only at very low pressures.)

  10. Boyle’s Law Calculations • A 1.5-L sample of gaseous CCl2F2 has a pressure of 56 torr. If the pressure is changed to 150 torr, will the volume of the gas increase or decrease? What will the new volume be? • Decrease • P1 = 56 torr • P2 = 150 torr • V1 = 1.5 L • V2 = ? V1P1 = V2P2 V2 = V1P1/P2 V2 = (1.5 L)(56 torr)/(150 torr) V2 = 0.56 L

  11. Boyle’s Law Calculations • In an automobile engine the initial cylinder volume is 0.725 L. After the piston moves up, the volume is 0.075 L. The mixture is 1.00 atm, what is the final pressure? • P1 = 1.00 atm • P2 = ? • V1 = 0.725 L • V2 = 0.075 L V1P1 = V2P2 P2 = V1P1/V2 P2 = (0.725 L)(1.00 atm)/(0.075 L) P2 = 9.7 atm Is this answer reasonable?

  12. A gas that strictly obeys Boyle’s Law is called an ideal gas.

  13. Plot of PV vs. P for several gases at pressures below 1 atm.

  14. Plot of V vs. T(oC) for several gases

  15. Volume of a gas increases as heat is added when pressure is held constant.

  16. Charles’s Law • The volume of a gas is directly proportional to temperature, and extrapolates to zero at zero Kelvin. • V = bT (P = constant) b = a proportionality constant

  17. Charles’s Law

  18. Charles’s Law Calculations • Consider a gas with a a volume of 0.675 L at 35 oC and 1 atm pressure. What is the temperature (in Co) of the gas when its volume is 0.535 L at 1 atm pressure? • V1 = 0.675 L • V2 = 0.535 L • T1 = 35 oC+ 273 = 308 K • T2 = ? V1/V2 = T1/T2 T2 = T1 V2/V1 T2 = (308 K)(0.535 L)/(0.675 L) T2 = 244 K -273 T2 = - 29 oC

  19. At constant temperature and pressure, increasing the moles of a gas increases its volume.

  20. Avogadro’s Law • For a gas at constant temperature and pressure, the volume is directly proportional to the number of moles of gas (at low pressures). • V = an • a = proportionality constant • V = volume of the gas • n = number of moles of gas

  21. AVOGADRO’S LAW V1/V2 = n1/n2

  22. AVOGADRO’S LAW A 12.2 L sample containing 0.50 mol of oxygen gas, O2, at a pressure of 1.00 atm and a temperature of 25 oC is converted to ozone, O3, at the same temperature and pressure, what will be the volume of the ozone? 3 O2(g) ---> 2 O3(g) (0.50 mol O2)(2 mol O3/3 mol O2) = 0.33 mol O3 V1 = 12.2 L V2 = ? n1 = 0.50 mol n2 = 0.33 mol V1/V2 = n1/n2 V2 = V1 n2/n1 V2 = (12.2 L)(0.33 mol)/(0.50 mol) V2 = 8.1 L

  23. COMBINED GAS LAW V1/ V2 = P2 T1/ P1 T2

  24. COMBINED GAS LAW What will be the new volume of a gas under the following conditions? V1 = 3.48 L V2 = ? P1 = 0.454 atm P2 = 0.616 atm T1 = - 15 oC + 273 = 258 K T2 = 36 oC + 273 T2= 309 K V1/ V2 = P2 T1/ P1 T2 V2 = V1P1T2/P2T1 V2 = (309 K)(0.454 atm)(3.48 L) (258 K)(0.616 atm) V2 = 3.07 L

  25. Pressure exerted by a gas increases as temperature increases provided volume remains constant.

  26. If the volume of a gas is held constant, then V1 / V2 = 1. Therefore: P1 / P2 = T1 / T2

  27. Ideal Gas Law • An equation of state for a gas. • “state” is the condition of the gas at a given time. • PV = nRT

  28. IDEAL GAS • 1. Molecules are infinitely far apart. • 2. Zero attractive forces exist between the molecules. • 3. Molecules are infinitely small--zero molecular volume. • What is an example of an ideal gas?

  29. REAL GAS • 1. Molecules are relatively far apart compared to their size. • 2. Very small attractive forces exist between molecules. • 3. The volume of the molecule is small compared to the distance between molecules. • What is an example of a real gas?

  30. Ideal Gas Law • PV = nRT • R = proportionality constant = 0.08206 L atm  mol • P = pressure in atm • V = volume in liters • n = moles • T = temperature in Kelvins • Holds closely at P < 1 atm

  31. Ideal Gas Law Calculations • A 1.5 mol sample of radon gas has a volume of 21.0 L at 33 oC. What is the pressure of the gas? • p = ? • V = 21.0 L • n = 1.5 mol • T = 33 oC + 273 • T = 306 K • R = 0.08206 Latm/molK pV = nRT p = nRT/V p = (1.5mol)(0.08206Latm/molK)(306K) (21.0L) p = 1.8 atm

  32. Ideal Gas Law Calculations • A sample of hydrogen gas, H2, has a volume of 8.56 L at a temperature of O oC and a pressure of 1.5 atm. Calculate the number of moles of hydrogen present. • p = 1.5 atm • V = 8.56 L • R = 0.08206 Latm/molK • n = ? • T = O oC + 273 • T = 273K pV = nRT n = pV/RT n = (1.5 atm)(8.56L) (0.08206 Latm/molK)(273K) n = 0.57 mol

  33. Standard Temperature and Pressure • “STP” • P = 1 atmosphere • T = C • The molar volume of an ideal gas is 22.42 liters at STP

  34. GAS STOICHIOMETRY • 1. Mass-Volume • 2. Volume-Volume

  35. Molar Volume • pV = nRT • V = nRT/p • V = (1.00 mol)(0.08206 Latm/molK)(273K) • (1.00 atm) • V = 22.4 L

  36. Gas StoichiometryNot at STP (Continued) • p = 1.00 atm • V = ? • n = 1.28 x 10-1 mol • R = 0.08206 Latm/molK • T = 25 oC + 273 = 298 K pV = nRT V = nRT/p V = (1.28 x 10-1mol)(0.08206Latm/molK)(298K) (1.00 atm) V = 3.13 L O2

  37. Gases at STP • A sample of nitrogen gas has a volume of 1.75 L at STP. How many moles of N2 are present? • (1.75L N2)(1.000 mol/22.4 L) = 7.81 x 10-2 mol N2

  38. Gas Stoichiometryat STP • Quicklime, CaO, is produced by heating calcium carbonate, CaCO3. Calculate the volume of CO2 produced at STP from the decomposition of 152 g of CaCO3. CaCO3(s) ---> CaO(s) + CO2(g) • (152g CaCO3)(1 mol/100.1g)(1mol CO2/1mol CaCO3) (22.4L/1mol) = 34.1L CO2 • Note: This method only works when the gas is at STP!!!!!

  39. Volume-Volume • If 25.0 L of hydrogen reacts with an excess of nitrogen gas, how much ammonia gas will be produced? All gases are measured at the same temperature and pressure. • 2N2(g) + 3H2(g) ----> 2NH3(g) • (25.0 L H2)(2 mol NH3/3 mol H2)= 16.7 L NH3

  40. MOLAR MASS OF A GAS • n = m/M • n = number of moles • m = mass • M = molar mass

  41. MOLAR MASS OF A GAS • P = mRT/VM • or • P = DRT/M • therefore: • M = DRT/P

  42. Molar Mass Calculations • M = ? d = 1.95 g/L • T = 27 oC + 273 p = 1.50 atm • T = 300. K R = 0.08206 Latm/mol K M = dRT/p M = (1.95g/L)(0.08206Latm/molK)(300.K) (1.5atm) M = 32.0 g/mol

  43. Dalton’s Law of Partial Pressures • For a mixture of gases in a container, PTotal = P1 + P2 + P3 + . . .

  44. Dalton’s Law of Partial Pressures Calculations • A mixture of nitrogen gas at a pressure of 1.25 atm, oxygen at 2.55 atm, and carbon dioxide at .33 atm would have what total pressure? • PTotal = P1 + P2 + P3 • PTotal = 1.25 atm + 2.55 atm + .33 atm • Ptotal = 4.13 atm

  45. Water Vapor Pressure • 2KClO3(s) ----> 2KCl(s) + 3O2(g) • When a sample of potassium chlorate is decomposed and the oxygen produced collected by water displacement, the oxygen has a volume of 0.650 L at a temperature of 22 oC. The combined pressure of the oxygen and water vapor is 754 torr (water vapor pressure at 22 oC is 21 torr). How many moles of oxygen are produced? • Pox= Ptotal - PHOH • Pox = 754 torr - 21 torr • pox = 733 torr

  46. MOLE FRACTION • -- the ratio of the number of moles of a given component in a mixture to the total number of moles of the mixture. • 1 = n1/ ntotal • 1 =V1/ Vtotal • 1 = P1 / Ptotal (volume & temperature constant)

  47. Kinetic Molecular Theory • 1. Volume of individual particles is  zero. • 2. Collisions of particles with container walls cause pressure exerted by gas. • 3. Particles exert no forces on each other. • 4. Average kinetic energy  Kelvin temperature of a gas.

  48. Plot of relative number of oxygen molecules with a given velocity at STP (Boltzmann Distribution).

  49. Plot of relative number of nitrogen molecules with a given velocity at three different temperatures.

  50. The Meaning of Temperature • Kelvin temperature is an index of the random motions of gas particles (higher T means greater motion.)

More Related