1. Calculate the volume of O 2 at STP required to burn 6.00 g of C 2 H 6 :

2. Stoichiometry with Gas Laws

3. Use the same rules for stoichiometry, but use PV = nRT for molar conversions (Steps 2 & 4)

4. Calculate the volume of carbon dioxide gas produced at 27 o C under 83.1 kPa pressure when 35 g of C 5 H 10 is burned in excess oxygen:

5. Calculate the mass of O 2 formed when 250 mL H 2 O at 127 o C under 83.1 kPa pressure is decomposed producing H 2 & O 2 :

6. A mixture of 10 % C 8 H 18 in O 2 is compressed to 8.31 mL in a piston at 27 o C under 750 kPa. Calculate the volume of released gases at 227 o C under 83.1 kPa.

7. Calculate the volume of HI (g) collected at 227 o C under 250 kPa pressure when 4.12 kg PI 3 reacts with xs water forming HI & H 3 PO 3.

8. Calculate the mass of CO 2 occupying 250 mL 167 o C under 400.0 kPa pressure:

9. Calculate the ratio of the velocities of Si & I 2 :

10. Determine the volume of NH 3 formed at 27 o C under 831 kPa when 2.0 x 10 27 molecules N 2 reacts with 4.0 kg of H 2 :

11. Determine the volume of O 2 released at 227 o C under 83.1 kPa when 32.0 kg of Fe 2 O 3 is purified making Fe & O 2

12. Calculate the mass of Iodine liberated when 831 mL F 2 at 27 o C under 150 kPa is bubbled through 150 ml of 0.40 M KI :

13. Calculate the mass of Mg used to generate 83.1 mL H 2 collected over water at 27 o C under 153.6 kPa when xs HCl is added to the Mg:

14. 23.4 g Al 2 (CO 3 ) 3 was added to 400. mL 1.0 M HCl generating AlCl 3 + CO 2 + H 2 O. Calculate the volume of gas collected at 27 o C under 450 kPa.

15. Calculate the concentration of all ions remaining in solution.

16. Draw the electron dot diagrams of elements number: 2, 4, 13, 24, 34, 37, 51, 52, 54, 77, 85, & 92

17. Classify Bonds K-ClCr-Cr P-SH-N Na-CaC-Cl Cs-FH-I