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

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Presentation transcript:

Kinetic Theory

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

Pressure

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

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

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

Gas Laws

State the Following Laws Boyle’s Law Charles’ Law Gay Lussac’s Law Dalton’s Law Graham’s Law

Boyle’s Law

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

Charles’ Law

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

Guy Lussac’s Law

The pressure and temp. of a gas at constant volume are directly proportioned P 1 P 2 T 1 T 2 = = K

Combined Gas Law

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

Common Sense

A gas’s volume is directly proportioned to its number of moles V 1 V 2 n 1 n 2 = = K

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

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

Ideal Gas Law PV = nRT

Dalton’s Law

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

Graham’s Law

The velocities of particles are inversely proportioned to the square root of their masses v 1 M 2 v 2 M 1 =

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

Calculate the volume of a gas at STP when it occupied mL at 227 o C under kPa pressure:

Calculate the volume of 3.0 moles of gas at -23 o C under 83.1 kPa pressure.

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

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

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

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

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

Integrated Formulas

Ideal Gas Law PV = nRT

Related Formulas m V m/n D or  = M =

M = m/n n = m/ M PV = nRT

mRT M mRT PV PV = M =

m V mRT PV D = M =

m V m RT V P D = M =

DRT P M P RT M = D =

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

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

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

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

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

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

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

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

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

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

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

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

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.