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Chapter 9 – Review Stoichiometry

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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

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