Substances that Exist as Gases

Transcription

1 Gases

2 Properties of Gases assume the volume and shape of their containers most compressible of the states of matter mix evenly and completely with other gases much lower density than other forms of matter

3 Substances that Exist as Gases

4 Elements that exist as gases at 25 C and 1 atm. The Noble gases (the Group 8A elements) are monatomic species; the other elements exist as diatomic molecules. Ozone (O 3 ) is also a gas.

5 Some substances found as gases at 1 atm and 25 ºC Elements H 2, N 2, O 2, O 3, F 2, Cl 2 He, Ne, Ar, Kr, Xe, Rn Compounds HF, HCl, HBr, Hl, CO, CO 2, NH 3, NO, NO 2, N 2 O, SO 2, H 2 S, HCN

6 Pressure of a Gas

7 Pressure The force exerted on an object divided by the surface area of the object; P = F A Any gas confined to a container is found to exert a pressure on the container.

8 Atmosospheric Pressure is the weight of air per unit of area. P = F A Gases 2012 Pearson Education, Inc.

9 SI Units of Pressure customary units 1.00 standard atm = 760 mm Hg = 760 torr SI units pressure = force/area pressure = Newton/m 2 = Pascal 1 standard atmosphere = Pa = kpa

10 vacuum atmospheric pressure mercury A Torricellian Barometer

11 vacuum 760 mm Hg (1 standard Atmosphere) atmospheric pressure mercury A Torricellian Barometer

12 The Gas Laws Boyle s Law Charles Law Avogadro s Law The Ideal Gas Law

13 The Gas Laws and the Scientific Method Observations Laws Theory Hypothesis Experiment Boyle Charles Avogadro Ideal Gas Kineticmolecular theory

14 Boyle s Law Robert Boyle

15 Boyle s Law The volume of a fixed quantity of gas at constant temperature is inversely proportional to the pressure. Gases 2012 Pearson Education, Inc.

16 Boyle s Data Pressure (mm Hg) Volume (arbitrary units)

17 Pressure (atm) P/ Volume (L) 2V

18 Pressure (mm Hg) Volume (arbitrary units) PV Boyle s Data

19 Boyle s Law at constant temperature, the volume of a constant amount of gas is inversely proportional to the pressure constant n, constant T PV = k

20 Plot of P versus V is a hyperbola PV = k P = (1/V ) k is of the form y = mx + b, which is the equation for a straight line

21 P P 0.6 at m 0.3 at m 2L 4L V (a) 1 V (b)

22 Charles s Law Jacques Charles

23 Charles s Law at constant pressure, the volume of a constant amount of gas is directly proportional to the absolute temperature constant n, constant P V = kt

24 50 He 40 CH 4 V(mL) º C H N 2 O t(ºc)

25 Celsius scale 5727 C Temperature at the surface of the sun Kelvin scale 6000 K 1064 C 100 C 37 C 0 C Melting point of gold Boiling point of water Body temperature Melting point of ice 1337 K K 310 K K 196 C Boiling point of N 2 77K C C Boiling point of He Lowest temperature (absolute zero) 4.2 K 0 K

26 Avogadro s Law Amadeo Avogadro ( )

27 Avogadro s Law The volume of a gas at constant temperature and pressure is directly proportional to the number of moles of the gas. Mathematically, this means V = kn Gases 2012 Pearson Education, Inc.

28 The Ideal-Gas Equation

29 The Ideal Gas Law PV = nrt constant n, constant T (Boyle s Law) constant n, constant P (Charles Law) constant P, constant T (Avogadro s Law)

30 The Ideal-Gas Law PV = nrt P is pressure in atmospheres V is volume in liters n is number of moles T is absolute temperature in Kelvins R is called the gas constant

31 An ideal gas is a hypothetical gas whose pressure-volume-temperature behavior can be completely accounted for by the ideal-gas equation.

32 Standard temperature and pressure PV = nrt standard conditions defined P = 1 atm T = 0ºC (273 K) STP

33 Standard Molar Volume The volume occupied by 1 mole of a gas at STP is L

34 The Gas Constant R The volume occupied by 1 mole of a gas at STP is L PV = nrt R = R = PV nt (1 atm) ( L) (1 mol) ( K) R = (L atm/mol K)

35 The constant of proportionality is known as R, the gas constant. The Gas Constant R Latm/molK Gases 2012 Pearson Education, Inc.

36 Example What is the volume occupied by 49.8 g of HCl at STP? 49.8 g x 1mol = mol g P = 1 atm T = 273 K nrt V = P (1.366 mol) ( L atm/mol K) (273K) V = 30.6 L 1 atm

37 Example What is the volume occupied by 49.8 g of HCl at STP? (alternative solution) 49.8 g n = = mol g/mol P = 1 atm T = 273 K V = x mol 22.4 L 1 mol V = 30.6 L

38 Example A compound has the empirical formula BH 3. At 27 º C, 74.3 ml of the gas exerted a pressure of 1.12 atm. If the mass of the gas was g, what is its molecular formula? PV = nrt n = PV RT

39 Example (cont.) A compound has the empirical formula BH 3. At 27 º C, 74.3 ml of the gas exerted a pressure of 1.12 atm. If the mass of the gas was g, what is its molecular formula? n = mol g = 27.6 g/mol mol BH 3 = 13.8 g / empirical formula B 2 H 6

40 The ideal gas law is often used to calculate the changes that will occur when the conditions of a gas are changed PV = nrt PV = nrt If nrt are constant If nrp are constant 1 P = ( nrt) nr V = V P ( ) PV = ( nrt ) = P 2 V V 2 2 = ( ) = V T nr P T T 2

41 The ideal gas law is often used to calculate the changes that will occur when the conditions of a gas are changed PV = nrt If PRT are constant RT V = ( ) V = n P RT ( ) P n = V 2 n 2 P T PV = nrt If nrv are constant P = nr ( ) V nr =( ) V = T P 2 T 2

42 Example A sample of oxygen gas initially at 0.97 atm is cooled from 21 º C to -68 º C at constant volume. What is its final pressure. PV = nrt P T nr =( ) V = P 2 T 2 P 1 P = 2 T 1 T 2

43 Example A sample of oxygen gas initially at 0.97 atm is cooled from 21 º C to -68 º C at constant volume. What is its final pressure. P 1 P = 2 T 1 T 2 (0.97 atm) 292 K = P K P 2 = 0.68 atm

44 Density Calculations

45 Density Calculations density = mass V n = mass Molar mass = g g/mol n V = P RT mass Molar mass(v) = P RT Therefore: density = P (Molar mass) RT

46 Example What is the density of UF 6 gas at 62 º C and 779mmHg? n = P 779mmHg V RT n = 760mmHg/atm V ( L atm/mol K) (335 K) = mol g x L 1 mol = 13.1g/L A common unit for gasses

47 Example n Cyanogen, empirical formula CN, is a gas with a density of g/l at 0ºC and 1 atm. What is its molecular formula? P V n = (1atm) (1 L) = RT ( L atm/mol K) (273K) 2.335g = mol = 52 g/mol Cyanogen 26g /mol (CN) C 2 N 2 = 2