1. In the compound AlCl₃, determine the:

a. number of Al atoms in one mole

b. number of Cl atoms in one mole

2. Calculate the molar mass of each of the following compounds:

a. AgNO₃

b. Mg(ClO)₂

c. Zn(IO₄)₂

d. CH₄

e. Na₂SO₄

3. Calculate in grams the mass of each of the following:

a. 4.61 mol AlCl₃

b. 0.615 mol Cr₂O₃

c. 0.158 mol IF₅

4. Calculate the number of items in each of the following

a. 2.3 moles of NaCl molecules

b. 1.8 moles of Ca atoms

c. 10.0 moles of MgBr₂

5. In an oxyacetylene welding torch, acetylene (C₂H₂) burns in pure oxygen with a very hot flame. The reaction is: 2 C₂H₂ + 5 O₂ → 4 CO₂ + 2 H₂O.

What is the mass of CO₂ that is produced if 20.0 grams of oxygen is allowed to react?

6. A Web site on fireworks provides directions for preparing potassium nitrate, KNO₃, by using potassium carbonate and ammonium nitrate according to the following equation:

K₂CO₃ + 2 NH₄NO₃ →  2 KNO₃ + CO₂ + H₂O + NH₃

The directions claim that one should "mix one kilogram of potassium carbonate with two kilograms of ammonium nitrate. The carbon dioxide and ammonia come off as gases, and the water can be evaporated, leaving two kilograms of pure potassium nitrate." Use information from this lesson to evaluate the claim.

7. State a response which describes where stoichiometry is used today.