Given the following UNBALANCED equation, determine how many moles of potassium chlorate are needed to produce 10.0 mol of oxygen gas.

2KClO3 (s) → 2KCl (s) + 3O2 (g)

10 mol O2 x 2 mol KClO3 = 6.67 mol KClO3

3 mol O2

How many moles of oxygen gas are produced if 5.25 mol of potassium chlorate decomposes?

5.25 mol KClO3 x 3 mol O2 = 7.88 mol O2

2 mol KClO3

2KClO3 (s) → 2KCl (s) + 3O2 (g)

How many moles of potassium chloride are produced if 3.70 g of KClO3 is decomposed?

3.70 g KClO3 x 1 mol KClO3 x 2 mol KCl = 0.0302 mol KCl 122.5 g KClO3 2 mol KClO3

2KClO3 (s) → 2KCl (s) + 3O2 (g)

2.5 g KClO3 x 1 mol KClO3 x 3 mol O2 x 32.0 g O2 = 122.5 g KClO3 2 mol KClO3 1 mol O2

= 0.980 g O2

How many grams of O2 are produced if 2.50 g of KClO3 is decomposed?

2KClO3 (s) → 2KCl (s) + 3O2 (g)

N2H4 (l) + O2 (g) → N2 (g) + 2H2O (g)

How many moles of water are produced when 20.0 g of hydrazine is reacted with 30.0 g of oxygen gas?