1. Acetylene, C₂H₂, can be synthesized in the laboratory as follows:

CaC₂(s) + 2H₂0(1) → C2H₂(g) + Ca(OH)₂(aq)

How much CaC₂ should be used to react with excess water in order to produce 17.5 L of C₂H₂, an ideal gas at STP?

2. Given:

2Na(s) + 2H₂O(1) → 2NaOH(aq) + H₂(g

Calculate the volume of H₂ produced from 10.0 kg of Na at STP.

3. Calculate the mole fraction of Ne in a 25.0-L vessel that contains 6.50 g of O₂, 10.6 g of Ar, 20.0 g of Ne, and 3.65 g of He at 75.0⁰C.

4. Calculate the total pressure of the mixture in Question 3.

5. What is the partial pressure of O₂ in the mixture in Question 3?

6. Given:
LiH(s) + H₂O(1) → LiOH(aq) + H₂(g)

Calculate the mass of LiH that should be used in order to collect 41.6 L of H₂ above water at 30.0^oC when the atmospheric pressure is 765 mmHg.

7. Briefly, state the objectives of the KMT.

8. Calculate the rms for molecular chlorine at 55.6^oC.

9. The time of effusion of 0.010 mol of He is 62 seconds at a certain temperature and pressure. How long will it take for the same amount of F2 to effuse under the same conditions?

10. A 65.0-g of O₂ is placed in a 7.50-L vessel at -25.0^oC. Calculate the pressure of oxygen in the vessel using the ideal gas law. Do the same calculation using the van der Waals equation. Do you see any deviation? Explain.