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

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

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

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Kinetic Theory

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

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Pressure

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

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

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Standard Pressure 101.3 kPa (to be changed) 1.00 Atm 760 mm Hg or Torrs 30.0 inches Hg 1013 millibars

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Gas Laws

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Boyles Law

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

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Charles Law

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

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Guy Lussacs Law

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

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Combined Gas Law

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

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

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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

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

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Ideal Gas Law PV = nRT

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

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

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

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

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Combined Gas Law PV = nRT

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

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

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

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Daltons Law

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

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The total pressure of a system is 120.0 kPa. The partial pressure of gas A is 112.0 kPa. Determine the pressure of gas B

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Grahams Law

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

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

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Calculate the volume of a gas at STP when it occupies 80.0 mL at 127 o C under 303.9 kPa pressure:

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

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

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Calculate the volume of a gas at STP when it occupies 80.0 mL at 127 o C under 303.9 kPa pressure:

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

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

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

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The total pressure of a system is 120.0 kPa. The partial pressure of gas A is 112.0 kPa. Determine the pressure of gas B

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The total pressure of a system is 150.0 kPa. The system contains 50 % A, 30 % B, & 20 % C. Determine the pressure of each gas.

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

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

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

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

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

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

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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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Chapter 11 The Behavior of Gases. Kinetic Theory Kinetic Theory – all molecules are in constant motion. –Collisions between gas molecules are perfectly.

Chapter 11 The Behavior of Gases. Kinetic Theory Kinetic Theory – all molecules are in constant motion. –Collisions between gas molecules are perfectly.

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