1. Chapter 10 review

2. Define the following: Hydrate Molecular formula Empirical formula
Percent composition
Mole

3. Find the atomic mass for the following atoms:
11. Cl
12. O
13. Fe

4. Find the molar mass for the following compounds:
14. CH2O
15. CaSO4
16. Na3PO4

5. Identify if the following problems are 1 or 2 steps
17. How many atoms are in moles of zinc?
18. How many moles of magnesium is 3.01 x 1022 atoms of magnesium?
19. How many atoms of nitrogen are in 1.2 grams of aspartame
20. Find the number of moles of argon in 452 g of argon
21. Find the mass of 1.00 x 1023 molecules of N2
22. What is the mass of 5 moles of Fe2O3

6. Solve the following molar conversions:
23. How many atoms are in moles of zinc?
24. How many moles of magnesium is 3.01 x 1022 atoms of magnesium?
25. Find the mass of 1.00 x 1023 molecules of N2

7. Solve the following percent composition problems for Nitrogen:
26. Mg(NO3)2
27. (NH4)2S

8. Solve the following empirical formula problem:
What’s the empirical formula of a molecule containing 65.5% carbon, 5.5% hydrogen, and 29.0% oxygen.
Element
Percent Composition C
65.5% H
5.5% O
29.0%

9. Solve the following molecular formula problem:
A compound with an empirical formula of C2H8N and a molar mass of 46 grams per mole. Find the molecular formula.

10. Determine the empirical formula for the compound whose percent composition.

11. Which samples have the same empirical formula?
Which substances have the same empirical formula?
Which samples have the same empirical formula?
Sample
Formula 1
CH3OH 2
CH2O 3
C6H12O6 4
C2H4O2

12. A hydrate of calcium chloride has a mass of 8. 52 g
A hydrate of calcium chloride has a mass of 8.52 g. This sample is heated until no water remains. The CaCl2 anhydrate has a mass of 5.60g. How many water molecules were attached to calcium chloride?