1. Chapter 9 – Review Stoichiometry
Milbank High School

2. Chapter 9 - Review
The calculation of quantities in chemical equations is called ____.
What is conserved in the following reaction: H2(g) + Cl2(g)  2HCl(g)
In every chemical reaction, what item(s) is/are conserved?

3. Chapter 9 - Review
What is true about the total number of reactants and the total number of products in the given equation: C5H12(l) + 8O2(g)  5CO2(g) + 6H2O(g)
In a chemical equation, the mass of the products is equal to _____.

4. Chapter 9 - Review
How many moles of Al are needed to react completely with 1.2 mol FeO?

5. Chapter 9 - Review
What are some reasons why actual yield is less than theoretical yield?
The reagent present in the smallest amount is ___ the limiting reagent.
For a given chemical reaction, the theoretical yield is ____ greater than the actual yield.

6. Chapter 9 - Review
When an equation is used to calculate the amount of product that will form, then the value obtained is called the _____.

7. Chapter 9 - Review
When two substances react to form products, the reactant which is used up is called the _____.
What mass of CaO (lime) is produced from 1.5 x 103 kg of CaCO3? CaCO3(s)  CaO(s) + CO2(g)

8. Chapter 9 - Review
Identify the limiting reagent, and volume of CO2 formed when 11.0 L CS2 reacts with 18.0 L O2 by: CS2(g) + 3 O2(g)  CO2(g) + 2SO2(g)

9. Chapter 9 - Review
How many liters of NH3 are needed to react completely with 30.0 L of NO (at STP)? 4 NH3(g) + 6NO(g)  5N2(g) + 6H2O(g)
The first step in most stoichiometry problems is to _____.

10. Chapter 9 Review Terms Actual yield Limiting reagent Theoretical yield
Stoichiometry
Percent yield
Excess reagent