1. PRACTICE PROBLEMS How many moles of glucose, C 6 H 12 O 6, can be burned when 10.0 mol of oxygen is available? C 6 H 12 O 6 (s) + 6O 2 (g)  6CO 2 (g) + 6H 2 O(l)

2. How many moles of H 3 PO 4 are produced when 71.0 g P 4 O 10 reacts completely to form H 3 PO 4 ?

3. How many liters of NH 3, at STP, will react with 5.3 g O 2 to form NO 2 and water? 4NH 3 (g) + 7O 2 (g)  4NO 2 + 6H 2 O(g)

4. If 8.00 mol of NH 3 reacted with 14.0 mol of O 2 how many moles of H 2 O will be produced? 4NH 3 (g) + 7O 2 (g)  4NO 2 + 6H 2 O(g)

5. How many liters of O 2 are needed to react completely with 45.0 L of H 2 S at STP? 2H 2 S(g) + 3O 2 (g)  2SO 2 (g) + 2H 2 O(g)

6. Hydrogen gas is produced when zinc reacts with hydrochloric acid. If the actual yield of this reaction is 85%, how many grams of zinc are needed to produce 112 L of H 2 at STP? Zn(s) + 2HCl(aq)  ZnCl 2 (s) + H 2 (g)

7. The decomposition of potassium chlorate yields oxygen gas. If the yield is 95%, how many grams of KClO 3 are needed to produce 10.0 L of O 2 ? 2KClO 3 (s)  2KCl(s) + 3O 2 (g)