1. Measuring the Pressure of a Gas and Gas Laws of Boyle, Charles and Avogadro Chemistry 142 B Autumn Quarter, 2004 J. B. Callis, Instructor Lecture #13

2. The Three States of Matter for the Element Bromine

3. Important Characteristics of Gases 1) Gases are highly compressible An external force compresses the gas sample and decreases its volume: removing the external force allows the gas volume to increase. 2) Gases are thermally expandable When a gas sample is heated, its volume increases. When it is cooled its volume decreases. 3) Gases have low viscosity Gases flow much easier than liquids or solids. 4) Most Gases have low densities Gas densities are on the order of grams per liter whereas liquids and solids are grams per cubic cm, 1000 times greater. 5) Gases are infinitely miscible Gases mix in any proportion such as in air, a mixture of many gases.

4. Helium He 4.0 Neon Ne 20.2 Argon Ar 39.9 Hydrogen H 2 2.0 Nitrogen N 2 28.0 Nitrogen Monoxide NO 30.0 Oxygen O 2 32.0 Hydrogen Chloride HCl 36.5 Ozone O 3 48.0 Ammonia NH 3 17.0 Methane CH 4 16.0 Substances that are Gases under Normal Conditions Substance Formula MM(g/mol)

5. Pressure of the Atmosphere Called “atmospheric pressure,” or the force exerted upon us by the atmosphere above. A measure of the weight of the atmosphere pressing down upon us. Measured using a barometer - A device that can weigh the atmosphere above us.

6. The Effect of Atmospheric Pressure on objects at the earth’s surface

7. A Mercury Barometer

8. Construct a Barometer using Water Density of water = Density of Mercury = Height of water column = H w H w = H w =

9. A Closed End Manometer

10. An Open ended Manometer

11. A J-tube similar to the one used by Boyle

12. Common Units of Pressure Unit Atmospheric Pressure Scientific Field pascal (Pa); 1.01325 x 10 5 Pa SI unit; physics, kilopascal(kPa) 101.325 kPa Chemistry atmosphere (atm) 1 atm* Chemistry millimeters of mercury 760 mmHg* Chemistry, medicine, ( mm Hg ) biology torr 760 torr* Chemistry pounds per square inch 14.7 lb/in 2 Engineering ( psi or lb/in 2 ) bar 1.01325 bar Meteorology, chemistry, physics

13. Problem 13-1: Converting Units of Pressure Problem: A chemist collects a sample of Carbon dioxide from the decomposition of limestone (CaCO 3 ) in a closed end manometer, the height of the mercury is 341.6 mm Hg. Calculate the CO 2 pressure in torr, atmospheres, and kilopascals. Plan: The pressure is in mmHg, so we use the conversion factors from The preceding table to find the pressure in the other units. Solution: (a) P CO2 (torr) = converting from mm Hg to torr: converting from torr to atm: (b) P CO2 ( atm) = converting from atm to kPa: (c) P CO2 (kPa) =

15. Boyle’s Law : P - V Relationship Pressure is inversely proportional to volume at fixed temperature and fixed amount: P = or V = or PV=K KVKV KPKP Where: P is the pressure exerted by the sample on the surroundings. V is the volume occupied by the sample. K is a constant of proportionality.

16. Problem 13-2: Applying Boyles Law Problem: A gas sample at a pressure of 1.23 atm has a volume of 15.8 cm 3, what will be the volume if the pressure is increased to 3.16 atm? Plan: We begin by converting the volume that is in cm 3 to mL and then to liters, then we do the pressure change to obtain the final volume. Solution: V 1 (cm 3 ) V 1 (ml) V 1 (L) V 2 (L) 1cm 3 = 1 mL 1000mL = 1L x P 1 /P 2 P 1 = 1.23 atm P 2 = 3.16 atm V 1 = 15.8 cm 3 V 2 = unknown T and n remain constant V 1 = V 2 =

17. Deviations From Boyle’s Law

18. Extrapolation of PV Data to Zero Pressure Yields Ideal Behavior

20. Charles’s Law : V - T Relationship Volume is directly proportional to temperature at fixed pressure and fixed amount: V = CT or = C V T Where: V is the volume occupied by the sample. T is the temperature in degrees Kelvin. C is a constant of proportionality.

21. Charles’s Law Behavior for Several Gases

22. Problem 13-3: Charles Law A sample of carbon monoxide, a poisonous gas, occupies 3.20 L at 125 o C. Calculate the temperature ( o C) at which the gas will occupy 1.54 L if the pressure remains constant. V 1 = T 1 = V 2 = T 2 = T 2 = T 2 = o C =

23. Problem 13-4: Amonton’s Law Problem: A copper tank is compressed to a pressure of 4.28 atm at a temperature of 0.185 o F. What will be the pressure if the temperature is raised to 95.6 o C? Plan: The volume of the tank is not changed, and we only have to deal with the temperature change, and the pressure, so convert to SI units, and calculate the change in pressure from the Temp.and Pressure change. Solution: T 1 = T 2 = P 2 =

25. Avogadro’s Law : V - n Relationship Volume is directly proportional to moles of gas at fixed pressure and temperature: V = Bn or = B V n Where: V is the volume occupied by the sample. n is the number of moles of gas. B is a constant of proportionality.

26. Problem 13-5: Avogadro’s Law Problem: Sulfur hexafluoride is a gas used to trace pollutant plumes in the atmosphere, if the volume of 2.67 g of SF 6 at 1.143 atm and 28.5 o C is 2.93 m 3, what will be the mass of SF 6 in a container whose volume is 543.9 m 3 at 1.143 atm and 28.5 o C? Plan: Since the temperature and pressure are the same, it is a V - n problem, so we can use Avogadro’s Law to calculate the moles of the gas, then use the molecular mass to calculate the mass of the gas. Solution: Molar mass SF 6 = 146.07 g/mol

28. Standard Temperature and Pressure (STP) A set of Standard conditions have been chosen to make it easier to understand the gas laws, and gas behavior. Standard Temperature = 0 0 C = 273.15 K Standard Pressure = 1 atmosphere = 760 mm Mercury At these “standard” conditions 1.0 mole of a gas will occupy a “standard molar volume”. Standard Molar Volume = 22.414 Liters = 22.4 L

31. Answers to Problems in Lecture #13 1.341.6 torr, 0.4495 atm, 45.54 kPa 2.0.00615 L 3.-81 o C 4.6.18 atm 5.496 g SF 6