1. GASES,LIQUIDS & SOLIDS GasesLiquidsSolids No fixed volume. Expand to fill container. Fixed volume. Conform to shape of container. Constrained by gravity Fixed volume & fixed dimensions. Resist deformation (changes of shape)

2. COMPOSITION OF AIR: Minor Components Also, variable amounts of: H 2 O (0 – 7 %) CO 2 (0.01 – 1 %) CO(0 – 0.000002 %) NO 2 (0 - 0.000002 %) SO 2 (0 - 0.0001 %) O 3 (0 – 0.000007 %)

3. COMPOSITION OF AIR: (contd.) Greenhouse Gases:

4. COMPOSITION OF AIR: (contd.) Greenhouse Gases: CO 2 & CH 4

5. COMPOSITION OF AIR: (contd.) Radon- Accumulates under houses

6. COMPOSITION OF AIR: (contd.) Radon- Accumulates under house Arises from radioactive decay of traces of Actinides, typically found in Granite!

7. NATURAL GAS CH 4 - FOUND WITH Oil deposits. He - Up to 4 % in natural gas deposits

8. WATER VAPOR H 2 O from evaporation of water from surfaces of Lakes, Rivers, Oceans (80 % of Earth’s surface)

9. GASES FROM HEATING SOLIDS CO 2 CaCO 3 CaO + CO 2 O 2 4NaNO 3 Na 2 O + N 2 + 5O 2 O 2 KClO 4 KCl + 2O 2 NH 3 NH 4 Cl NH 3 + HCl Also: Gases (H 2 ) from metals and acids, also from some metals and water (Li, Na).

10. GAS PRESSURE Results from gravitational force on Earth’s atmospheric gases (several miles deep). Measure with Barometer. P = Pressure = gdh –g = accel. due to gravity –d = density of liquid column –h = height of column

11. PRESSURE MEASUREMENTS 1 Atmosphere (atm.) = 760 mm Hg d H 2 O = 1.00 g cm -3 d Hg = 13.6 g cm -3 For same P (= 1 atm. = 760 mm Hg = 760 x 13.6 mm H 2 O = 10.336 m = 33.91 ft H 2 O

12. PRESSURE MEASUREMENTS Pressure usually meaured in: (a) mm Hg (torr) 1 atm. – 760 mm Hg (b) Pa (PASCALS) = N m -2 = kg m -1 s -1 1 Atm. = 101.325 kPa 1 bar = 105 kPa = approx. 1 atm. (= 0.9869 atm.)

13. PRESSURE MEASUREMENTS Common measure (engineering): –psi = Pounds per square inch psig= Pounds per square inch, gauge –( add current atmospheric pressure to convert to Absolute pressure) –1 atm. = 14.7 psi

14. TEMPERATURE C(elcius) vs. F(ahrenheit) F = C x 9/5 + 32 C = (F-32) x 5/9 Absolute Temperature (K) At 0K, all gases have 0 volume K = 0 C + 273.15

15. IDEAL GAS LAW PV = Nrt or P 1 V 1 = P 2 V 2 n 1 T 1 n 2 T 2

16. AVOGADRO’S LAW 1 L. of all gases contains the same no. of molecules at the same T & P At STP (= 1 atmos. And 0 C), 1 mol. of any gas occupies 22.4 L Aso R= 1 atm. x 22.4 L 1 mol x 273.15K = 0.082057 L. atm.mol -1 K -1

17. UNIVERSAL GAS CONSTANT R = 0.082057 L. atm.mol -1 K -1 or R = 8.3145 J mol -1 K -1

18. GAS DENSITY & MOLAR MASS