1. Given the following UNBALANCED equation, determine how many moles of potassium chlorate are needed to produce 10.0 mol of oxygen gas. 2KClO 3 (s) → 2KCl (s) + 3O 2 (g) 10 mol O 2 x 2 mol KClO 3 = 6.67 mol KClO 3 3 mol O 2

2. How many moles of oxygen gas are produced if 5.25 mol of potassium chlorate decomposes? 5.25 mol KClO 3 x 3 mol O 2 = 7.88 mol O 2 2 mol KClO 3 2KClO 3 (s) → 2KCl (s) + 3O 2 (g)

3. How many moles of potassium chloride are produced if 3.70 g of KClO 3 is decomposed? 3.70 g KClO 3 x 1 mol KClO 3 x 2 mol KCl = 0.0302 mol KCl 122.5 g KClO 3 2 mol KClO 3 2KClO 3 (s) → 2KCl (s) + 3O 2 (g)

4. 2.5 g KClO 3 x 1 mol KClO 3 x 3 mol O 2 x 32.0 g O 2 = 122.5 g KClO 3 2 mol KClO 3 1 mol O 2 = 0.980 g O 2 How many grams of O 2 are produced if 2.50 g of KClO 3 is decomposed? 2KClO 3 (s) → 2KCl (s) + 3O 2 (g)

5. 20.0 g N 2 H 4 x 1 mol N 2 H 4 x 2 mol H 2 O = 1.23 mol H 2 O 32.06 g N 2 H 4 1 mol N 2 H 4 30.0 g O 2 x 1 mol O 2 x 2 mol H 2 O = 1.88 mol H 2 O 32.00 g O 2 1 mol O 2 N 2 H 4 (l) + O 2 (g) → N 2 (g) + 2H 2 O (g) How many moles of water are produced when 20.0 g of hydrazine is reacted with 30.0 g of oxygen gas?