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State the Following Laws Boyles Law Charles Law Gay Lussacs Law Daltons Law Grahams Law.

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Presentation on theme: "State the Following Laws Boyles Law Charles Law Gay Lussacs Law Daltons Law Grahams Law."— Presentation transcript:

1 State the Following Laws Boyles Law Charles Law Gay Lussacs Law Daltons Law Grahams Law

2 Drill: Calculate the volume at STP of CO 2 released when 23.4 g of aluminum carbonate is decomposed 75 % through heat

3 AP Test Changes No Choices in Problems Only 3 reactions with predicting products –Balance rxns –No choices –Explain rxns

4 Kinetic Theory

5 All matter is made up of tiny particles The particles are in constant motion All collisions are elastic

6 Pressure

7 Force per unit area Caused by collisions against a surface Gas measured in pressure

8 Units of Pressure kPa: kilopascal (Std Unit) Pascal: newton/sq. meter Atmosphere (Atm): mm Hg:

9 Standard Pressure kPa (to be changed) 1.00 Atm 760 mm Hg or Torrs 30.0 inches Hg 1013 millibars

10 Gas Laws

11 Boyles Law

12 The pressure & volume of a gas at constant temperature are inversely proportioned P 1 V 1 = P 2 V 2 = K

13 Charles Law

14 The volume and temperature of a gas at constant pressure are directly proportioned V 1 /T 1 = V 2 /T 2 = K

15 Guy Lussacs Law

16 The Pressure and temperature of a gas at constant volume are directly proportioned P 1 /T 1 = P 2 /T 2 = K

17 Combined Gas Law

18 Combination of the three formulas P 1 V 1 /T 1 = P 2 V 2 /T 2

19 Calculate the new volume of 5.0 L of gas when its pressure is doubled and its temperature is tripled:

20 Common Sense The volume of a gas is directly proportioned to the number of moles of gas V 1 /n 1 = V 2 /n 2 = K

21 New Combination P 1 V 1 /n 1 T 1 = P 2 V 2 /n 2 T 2 = K

22 Ideal Gas Law PV = nRT

23 Calculate the volume of 2.0 moles of gas at 77 o C under 83.1 kPa pressure.

24 Calculate the number of moles of gas occupying 831 mL under 250 kpa at 227 o C

25 Calculate the number of moles of gas occupying 831 mL under 80.0 kPa at 127 o C

26 Calculate the mass of CO 2 occupying 83.1 L under 25 GPa at 227 o C

27 Combined Gas Law PV = nRT

28 Related Formulas m V m/n D or = MW =

29 Calculate the molecular mass of 5.0 g of gas occupying 831 L under 250 Mpa at 227 o C

30 Calculate the density of carbon dioxide at 27 o C under 83.1 kPa pressure

31 Daltons Law

32 The total pressure = the sum of the partial pressures P T = P 1 + P 2 + etc

33 The total pressure of a system is kPa. The partial pressure of gas A is kPa. Determine the pressure of gas B

34 Grahams Law

35 The velocity of a particle is inversely proportioned to the square root of its mass v 1 /v 2 = M 2 / M 1

36 Drill: Calculate the ratio of the velocities of He gas to HCl gas:

37 Calculate the volume of a gas at STP when it occupies 80.0 mL at 127 o C under kPa pressure:

38 Drill:Calculate the volume of 4.0 moles of gas under 83.1 kPa pressure at 127 o C:

39 Calculate the mass of 831 mL of CO 2 at 27 o C under 150 kPa pressure:

40 Calculate the volume of a gas at STP when it occupies 80.0 mL at 127 o C under kPa pressure:

41 Calculate the volume of 4.0 moles of gas under 83.1 kPa pressure at 127 o C:

42 Calculate the molecular mass of 50 g of gas occupying 831 L under 250 MPa at 227 o C

43 Calculate the mass of 831 mL of CO 2 at 167 o C under 150 kPa pressure:

44 The total pressure of a system is kPa. The partial pressure of gas A is kPa. Determine the pressure of gas B

45 The total pressure of a system is kPa. The system contains 50 % A, 30 % B, & 20 % C. Determine the pressure of each gas.

46 Drill: Calculate the mass of CO 2 occupying 83.1 L under 25 MPa at 477 o C

47 Calculate the density of carbon dioxide at 27 o C under 83.1 kPa pressure

48 Calculate the ratio of the velocities of He gas to HCl gas:

49 Calculate the velocity HBr when the velocity Be is 270 m/s:

50 Calculate the final volume that 3.0 L of gas will obtain when the absolute temperature is tripled & the pressure is halved.

51 Calculate the mass of CO occupying 831 kL at 227 o C under 2.50 Mpa pressure.

52 Calculate the volume of H 2 formed at 27 o C under 150 kPa when 6.8 mg NH 3 decomposes making N 2 & H 2.


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