Practice Problems, Ch 10
Section 10.1:
1. 342.3 g/mol
2a. 208.2 g/mol
2b. 352.0 g/mol
3a. 158.0 g/mol
3b. 310.2 g/mol
4. 5.85 mol H2O
5. 3.6e23 atoms
6. 32.0 g
Section 10.2
1a. 180.2 g/mol
1b. 84.0 g/mol
1c. 96.2 g/mol
1d. 153.2 g/mol
2a. 1.8e3 g
2b. 26 g
2c. 3.20e-2 g
2d. 0.480 g
5c. 1.08e-3 mol
5d. 1.98e-5 mol
2e. 1.43e2 g
3. 1.87e2 g
4. 204.1 g
5a. 4.9e-3 mol
5b. 9.10e-2 mol
5e. 1.97e-5 mol
6. 5.43 mol
7. 15.1 g
8. 59.6 L CH4
9. 6.03 mol NH3
Section 10.3
1. 10.1% C, 0.79% H, 89.1% Cl
2. 31.3% Sn, 68.7% Cl
3. 81.7% C, 18.3% H
4. 19.8 g of carbon
5. 13.2 g of Al
6. 15.11 g of Fe
7a. CCl4
7b. CHCl3
Important Note: This worksheet does not provide
sufficient practice with empirical formula calculations or
laboratory applications of the mole. Review the in-class
worksheet that featured numerous percent composition,
empirical formula, and molecular formula problems. Also
review the laboratory work we did (and the associated
vocabulary) with hydrated salts. That work included a prelab practice set and then real-time lab work to determine
the formula of a hydrates sale and the percent by mass of
water in the hydrated salt. Laboratory work also included
percent error analysis.