1. Gas Laws #1 ODDS 1) 396 mL = 0.396 L 3) 10.92 L 5) 24.3 lb/in2
X(N2) =(4moles/9moles) = P(N2) = torr
X(O2) = .333 P(O2) = torr
X(He) = .222 P(He) = torr
11) 48.0 mL

2. Gas Laws #1 EVENS
2) 670 L or 673 L (since all have 3 sig fig except 740 torr)
4) 0.45 moles
6) 446 moles He
2.50 x103 mL = 2.48 L Boyle’s Law
P(N2) = 559 mm Hg
P(O2) = 118 mm Hg
P(CO2) = 27 mm Hg
P(H2O) = 47 mm Hg
12) 650 kPa (670kPa?)

3. 529 mL (or L)
133 L
0.225 Atm / CH4
3.38 L
3.1 x1023 molecules

4. Gas Laws Practice #2 1. 529 mL (0.529 L) 2. 808 torr (1.06 atm)
CH4 has greatest partial pressure
H2S (g) + 3 O2 (g) → 2 SO2 (g) + 2 H2O (g)
@ 11.5 g SO2

5. Gas Laws Practice #2 3.38 L 736 mm Hg (0.968 atm) 0.160 g H2
3.1 x1023 molecules
10) SF6 / sulfur hexafluoride

6. Gas Laws #2 EVENS
1.06 atm
33.27 atm
2 H2S (g) + 3 O2 (g) → 2 SO2 (g) + 2 H2O (g)
12 g SO2
736 mm Hg
0.160 g H2
10) SF6 / sulfur hexafluoride

7. Diffusion Packet Section Review #3: 17 g/mole #4: 256:1
#4: 256:1
#5: BrF, NO2, HCl, H2O, He
#6: 128 g/mol, HI
Chapter Review
#56: (a) 3.72, (b) 1.37
#57: 3.16
#58: 341 m/s

8. Gas Laws #3 ODDS 12 mL –223 °C 5a) 748 mm Hg 5b) 0.454 g O2
17.1 g NaCN
10.6 mL H2O

9. Gas Laws #3 EVENS 8.13 L 42.1 g/mol 247 kPa 0.0349 g C8H18
10a) 2.53 g NaBH4
10b) 1.80 L

10. Gas Laws #4 3500 L 8276 L 113.7 K 0.24 L 188 g/mol C2H4Br2 39.2 L
a) 12 atm
b) 6.0 atm
3.41 g/L
8) a) 736 mm Hg
b) 14,300 g Ga

11. Gas Laws #4 EVENS 39.2 L a) 12 atm b) 6.0 atm 3.41 g/L 8) a) 736 mm Hg
b) 14,300 g Ga

12. Gas Laws Review 0.30 atm All 3 have the same Helium C4H8
C4H8 + 6 O2 → 4 CO2 + 4 H2O
2.91 L CO2

13. Another Gas Laws Review
146 g/mol
15.2 Liters
(a) torr (b)1490 torr
10.5 Liters
C4H8
112 g/mol / C3H6Cl2
(a) 800 torr (b) moles (c) all the same (d) neon since it has the lowest mass
4.71 Liters
3.22 Atm