Reference no: EM131281883
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 30.0oC when the atmospheric pressure is 765 mmHg.
7. Briefly, state the objectives of the KMT.
8. Calculate the rms for molecular chlorine at 55.6oC.
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 -25.0oC. 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.
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Calculate the total pressure of the mixture
: 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. Calculate the total pressure of the mixture in Question 3.
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