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Chapter 9 – Review Stoichiometry Milbank High School.

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Presentation on theme: "Chapter 9 – Review Stoichiometry Milbank High School."— Presentation transcript:

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: H 2(g) + Cl 2(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: C 5 H 12(l) + 8O 2(g)  5CO 2(g) + 6H 2 O (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 10 3 kg of CaCO 3 ? CaCO 3(s)  CaO (s) + CO 2(g)

8 Chapter 9 - Review Identify the limiting reagent, and volume of CO 2 formed when 11.0 L CS 2 reacts with 18.0 L O 2 by: CS 2(g) + 3 O 2(g)  CO 2(g) + 2SO 2(g)

9 Chapter 9 - Review How many liters of NH 3 are needed to react completely with 30.0 L of NO (at STP)? 4 NH 3(g) + 6NO (g)  5N 2(g) + 6H 2 O (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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