Give the following reaction: 

FeO(s) + CO(g) → Fe(s) + CO2(g) 

a. How many moles of CO are needed to react with 54.2 g of FeO

b. What is the mass of Fe solid produced by 54.2 g of FeO

2. Give the following reaction: 

ammonium nitrate → dinitrogen monoxide + water

a. Write a complete balanced chemical equation.

b. Calculate the number of molecules of water produced by 11.2g of ammonium nitrate

3. When potassium chlorate is heated, it decomposes to potassium chloride and oxygen gas.

Write a balanced chemical equation. Calculate the mass of oxygen gas produced by 0.25 kg of potassium

chlorate.

4. Given the following balance chemical equation: 

Fe2O3 + 3H2SO4 → Fe2(SO4)3 + 3H2O 

21.6g of Fe2O3 is placed in this reaction 

a) How many grams of H2SO4 required to react fully with 21.6g of Fe2O3? 

b) How many mole of Fe2(SO4)3 will be produced in this reaction, given 21.6g of Fe2O3? 

c) How many molecules of Fe2(SO4)3 will be produced in this reaction? 

(Hint: use answer from b) 

5. Given the following balance chemical equation: 

2 AgNO3 (aq) + CaCl2 (aq) → Ca(NO3)2 (aq) + 2 AgCl (s)

15.0 g of AgNO3 and 15.0 g of CaCl2 are placed in this reaction. 

a) Which one is the limiting reactant? Which one is the excess reactant? Show calculation on the mass of 

product produced to support your answer.

b) How many grams of AgCl (s) can be produced in this reaction? 

c) If at the end of the experiment, you collected 10.7g of AgCl (s), what is the percent yield? 

d) How many grams of the excess reactant is left over?