EXERCISES
1. From the following data calculate the atomic weight of sulphur. The equivalent, as obtained by an analysis of sulphur dioxide, is 16.03. The densities and compositions of a number of compounds containing sulphur are as follows:
| NAME | DENSITY | COMPOSITION BY PERCENTAGE | ||
| Hydrosulphuric acid | 1.1791 | S = 94.11 | H = 5.89 | |
| Sulphur dioxide | 2.222 | S = 50.05 | O = 49.95 | |
| Sulphur trioxide | 2.74 | S = 40.05 | O = 59.95 | |
| Sulphur chloride | 4.70 | S = 47.48 | Cl = 52.52 | |
| Sulphuryl chloride | 4.64 | S = 23.75 | Cl = 52.53 | O = 23.70 |
| Carbon disulphide | 2.68 | S = 84.24 | C = 15.76 | |
2. Calculate the formulas for compounds of the following compositions:
| MOLECULAR WEIGHT | |||
| (1) S = 39.07% | O = 58.49% | H = 2.44% | 81.0 |
| (2) Ca = 29.40 | S = 23.56 | O = 47.04 | 136.2 |
| (3) K = 38.67 | N = 13.88 | O = 47.45 | 101.2 |
3. The molecular weight of ammonia is 17.06; of sulphur dioxide is 64.06; of chlorine is 70.9. From the molecular weight calculate the weight of 1 l. of each of these gases. Compare your results with the table on the back cover of the book.
4. From the molecular weight of the same gases calculate the density of each, referred to air as a standard.
5. A mixture of 50 cc. of carbon monoxide and 50 cc. of oxygen was exploded in a eudiometer, (a) What gases remained in the tube after the explosion? (b) What was the volume of each?
6. In what proportion must acetylene and oxygen be mixed to produce the greatest explosion?
7. Solve Problem 18, Chapter XVII, without using molecular weights. Compare your results.