Here are the answers to the review. Watch out for sig figs! Let me know tomorrow if you have any questions BEFORE 3rd hour. Also, let me know if you find any errors... but I'm pretty much perfect at this... usually... sometimes...

a.

b.

c.

d.

e.

f.

1. V2 =

2. T2 =

3. Volume will increase by 4x due to temp, but decrease by 3x due to pressure, so total change is

4. P2 =

5. V2 =

6. V =

7. P =

8. m = 3.8 g

9. mol = 78.125 mol; P =

10. If 1.00 g Br2 gas, then mol = 0.00626 mol = 0.171 L; D =

11. If 1.00 g Ar, then mol = 0.025 mol = 0.606 L; D =

12. If 100 g of Freon, then 16.3 L = 0.727 mol; Molar Mass =

13. Empirical formula = NO2; Molar Mass = 92.02 g/mol; Molecular Formula is

14. Partial Pressure of Ar = 0.469 atm

15. Pressure of H2 = 0.877 atm; mol H2 = 0.283; m =

16. If 1.00 g of air; D =

17. CO2 = 0.45 mol; Volume CO2 =

18. O2 = 0.274 mol; Volume O2 =

19. H2 = 0.0997 mol; Volume H2 =

20. 1.00 L N2 = 1000 mL = 807 g N2 = 28.8 mol; Volume N2 gas =

**Part 1:**a.

**1010 torr**b.

**0.757 atm**c.

**32400 torr**d.

**36100 Pa**e.

**5.66 mm Hg**f.

**220 kPa****Part 2:**1. V2 =

**17.2 L**2. T2 =

**586 K**or**313 C**3. Volume will increase by 4x due to temp, but decrease by 3x due to pressure, so total change is

**4/3**.4. P2 =

**0.7 atm**5. V2 =

**0.305 L**6. V =

**54 L**7. P =

**5180 mm Hg**8. m = 3.8 g

9. mol = 78.125 mol; P =

**47 atm**10. If 1.00 g Br2 gas, then mol = 0.00626 mol = 0.171 L; D =

**5.86 g/L**11. If 1.00 g Ar, then mol = 0.025 mol = 0.606 L; D =

**1.7 g/L**12. If 100 g of Freon, then 16.3 L = 0.727 mol; Molar Mass =

**137 g/mol**13. Empirical formula = NO2; Molar Mass = 92.02 g/mol; Molecular Formula is

**N2O4**!14. Partial Pressure of Ar = 0.469 atm

15. Pressure of H2 = 0.877 atm; mol H2 = 0.283; m =

**0.57 g**16. If 1.00 g of air; D =

**1.77 g/L**17. CO2 = 0.45 mol; Volume CO2 =

**34.8 L**18. O2 = 0.274 mol; Volume O2 =

**11.7 L**19. H2 = 0.0997 mol; Volume H2 =

**2.9 L**20. 1.00 L N2 = 1000 mL = 807 g N2 = 28.8 mol; Volume N2 gas =

**705 L**