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Section 11-1 Section 11.1 Defining Stoichiometry Describe the types of relationships indicated by a balanced chemical equation. reactant: the starting.

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Presentation on theme: "Section 11-1 Section 11.1 Defining Stoichiometry Describe the types of relationships indicated by a balanced chemical equation. reactant: the starting."— Presentation transcript:

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2 Section 11-1 Section 11.1 Defining Stoichiometry Describe the types of relationships indicated by a balanced chemical equation. reactant: the starting substance in a chemical reaction stoichiometry mole ratio State the mole ratios from a balanced chemical equation. The amount of each reactant present at the start of a chemical reaction determines how much product can form.

3 Composition Stoichiometry Composition Stoichiometry: –Mass relationships of elements in compounds –Example: Percent composition of hydrogen in water?

4 Section 11-1 Particle and Mole Relationships Why does a reaction stop? Reaction Stoichiometry is the study of quantitative relationships between the amounts of reactants used and amounts of products formed by a chemical reaction.Reaction Stoichiometry Quantitative vs qualitative

5 Section 11-1 Particle and Mole Relationships (cont.) Stoichiometry is based on the law of conservation of mass. The mass of reactants must equal the mass of the products.

6 Section 11-1

7 Particle and Mole Relationships (cont.) A ________________is a ratio between the numbers of moles of any two substances in a balanced equation.

8 Section 11-2 Section 11.2 Stoichiometric Calculations List the sequence of steps used in solving stoichiometric problems. chemical reaction: a process in which the atoms of one or more substances are rearranged to form different substances Solve stoichiometric problems. The solution to every stoichiometric problem requires a balanced chemical equation.

9 Section 11-2 Using Stoichiometry All stoichiometric calculations begins with a balanced chemical equation. 4Fe(s) + 3O 2 (g)  2Fe 2 O 3 (s)

10 4 Types of Reaction Stoichiometry Problems Mole – Mole (1 step) Mole – Mass (2 steps) Mass – Mole (2 steps) Mass – Mass (3 steps)

11 Section 11-2 Mole Mountain (2)

12 Mole - Mole Mole to Mole CO 2 + Li(OH) → Li 2 CO 3 + H 2 O How many moles of Lithium hydroxide are required to react with 30 mol of carbon dioxide?

13 Mole - Mass Mole to Mass CO 2 + H 2 O → C 6 H 12 O 6 + O 2 3.00 mol of water to start. How many grams of glucose can be produced?

14 Mass - Mole Mass to Mole C + SO 2 → CS 2 + CO If 8.00 grams of sulfur dioxide reacts, how many moles of carbon disulfide are produced?

15 Mass - Mass Mass to Mass Sn + HF → SnF 2 + H 2 How many grams of tin (II) fluoride are produced from reacting 30.00 grams of HF?

16 Section 11-3 Section 11.3 Limiting Reactants Identify the limiting reactant in a chemical equation. molar mass: the mass in grams of one mole of any pure substance Identify the excess reactant, and calculate the amount remaining after the reaction is complete. Calculate the mass of a product when the amounts of more than one reactant are given.

17 Section 11-3 Section 11.3 Limiting Reactants (cont.) limiting reactant excess reactant A chemical reaction stops when one of the reactants is used up.

18 Section 11-3 Why do reactions stop? Reactions proceed until one of the reactants is used up and one is left in excess. The ______________________limits the extent of the reaction and, thereby, determines the amount of product formed. The __________________________are all the leftover unused reactants.

19 If I have 400 tires, 150 engines, 200 steering wheels, and 300 bucket seats (2 per car), how many complete cars could I make? What is the limiting reactant? What are the excess reactants?

20 Section 11-3 Why do reactions stop? (cont.) Determining the limiting reactant is important because the amount of the product formed depends on this reactant.

21 Section 11-3 Calculating the Product when a Reactant is Limiting S 8 (l) + 8Cl 2 (g) → 4S 2 Cl 4 (l) 200.0g S and 100.0g Cl 2 Determine which is the limiting reactant

22 Section 11-3 Calculating the Product when a Reactant is Limiting (cont.) Using an excess reactant can speed up the reaction. Using an excess reactant can drive a reaction to completion.

23 Section 11-4 Section 11.4 Percent Yield Calculate the theoretical yield of a chemical reaction from data. process: a series of actions or operations theoretical yield actual yield percent yield Determine the percent yield for a chemical reaction. Percent yield is a measure of the efficiency of a chemical reaction.

24 Section 11-4 How much product? Laboratory reactions do not always produce the calculated amount of products. Reactants stick to containers. Competing reactions form other products.

25 Section 11-4 How much product? (cont.) The ___________________is the maximum amount of product that can be produced from a given amount of reactant. The ____________________is the amount of product actually produced when the chemical reaction is carried out in an experiment.

26 The percent yield of a product is the ratio of the actual yield expressed as a percent.percent yield

27 Section 11-4 Percent Yield in the Marketplace Percent yield is important in the cost effectiveness of many industrial manufacturing processes. If you are supposed to make 100 pounds of aspirin, and only produce 50 pounds, the company has now lost money.


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