A. Equations are recipes: It tells the chemists what amounts of reactants to mix and what amounts of products to expect. B. What is Stoichiometry?
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1 Chapter 9 Stoichiometry NAME 9.1 The Arithmetic of Equations A. Equations are recipes: It tells the chemists what amounts of reactants to mix and what amounts of products to expect. B. What is Stoichiometry? C. Let s examine stoichiometry a bit closer by looking at the production of ammonia from it s elements: Write the equation below: Valuable information can be derived from this equation: Write sentences to describe the equation - 1. In terms of PARTICLES 2. In terms of MOLES 3. In terms of MASS 4. In terms of VOLUME(for gases only!) D. What was conserved (stayed the same from left to right) in this equation? (2 answers) Practice Problems: 1. a. Write the equation for the complete combustion of liquid ethanol, C 2 H 5 OH: b. Interpret the equation in terms of numbers of molecules c. Interpret the equation in terms of moles 1
2 d. Interpret the equation in terms of mass e. Why can t this problem be interpreted in terms of volume? 2. a. Write the balanced equation for the single-displacement reaction of solid potassium metal reaction with liquid water: b. Interpret this equation in terms of: i. Interaction particles- ii. moles iii. mass iv. volume (if allowed) 9.2 Chemical Calculations A. Mole-Mole Calculations: The heart of the stoichiometry problem Think WANT OVER GIVEN Example Problem: Rewrite the balanced equation for the production of ammonia from its elements: How many moles of ammonia are produced when 0.6 mol of nitrogen react with hydrogen? 2
3 Example Problem: Write the equation of aluminum oxide from its elements. How many moles of aluminum are needed to form 3.7 moles of aluminum oxide? How many moles of oxygen are required to react completely with 14.8 mole of aluminum? How many moles of aluminum oxide are formed when 0.78 mol of oxygen reacts with aluminum? B. Mass-Mass Calculations Example Problem: Rewrite the equation for the production of ammonia: Calculate the number of grams of ammonia produced by the reaction of 5.4 grams of hydrogen with an excess of nitrogen. Example Problem: Write the balanced chemical equation for the decomposition for potassium chlorate. Calculate the number of grams of reactant necessary to produce 50 grams of potassium chloride. How many grams of oxygen gas are produced when you decompose 15 grams of potassium chlorate? 3
4 How many MOLES of each product are produced when 10 grams of potassium chlorate are heated? How many grams of each product are produced when 2.5 moles of reactant are used? C. Other Stoichiometric Calculations The Stoichiometry Road Map *With your knowledge of conversion factors and the problem-solving diagram, you can solve a variety of stoichiometric problems. Example Problem: How many molecules of oxygen are produced when a sample of 29.2 grams of water is decomposed by electrolysis? Example Problem: How many liters of oxygen are produced by the decomposition of 6.54 grams of potassium chlorate? Example Problem: Assuming STP, how many liters of oxygen gas are needed to produce 19.8 L sulfur trioxide according to this balanced equation? 2SO 2 (g) + O 2 (g) 2SO 3 (g) Example Problem: Nitrogen monoxide and oxygen gas combine to form the brown gas nitrogen dioxide. How many milliliters of nitrogen dioxide are produced when 3.4 milliliters of oxygen react with an excess of nitrogen monoxide? Assume STP conditions. 4
5 Practice Problem Set: 1. Isopropyl alcohol (C 3 H 7 OH) completely combusts. Write the balanced equation Calculate the moles of oxygen needed to react with 3.4 mol of C 3 H 7 OH. Find the moles of each product formed when 3.4 mol of C 3 H 7 OH reacts with oxygen. 2. Acetylene gas completely combusts. Write the balanced equation How many grams of each product are produced when 52 grams of acetylene burns? How many grams of oxygen are required to burn 52 grams of acetylene? Show how this problem obeys the law of conservation of mass: 3. Tin II fluoride, formerly found in many kinds of toothpaste, is formed by the single replacement reaction between tin metal and hydrogen fluoride gas. Write this complete balanced equation. How many liters of HF are needed to produce 9.4 Liters H2 at STP? How many molecules of H2 are produced by the reaction of tin with 20 Liters HF at STP? How many grams of tin II fluoride can be made by reaction 7.42 E 24 molecules of HF with tin? 5
6 Section 9.3 Limiting Reagent and Percent Yield Define Limiting Reagent- Define Excess Reagent- Write the equation for the production of ammonia: This represents the most efficient recipe that a chemist can follow. Find the Limiting Reagent if the reaction was run with 2 moles of nitrogen and 3 moles of hydrogen: Example Problem: Sodium chloride can be prepared by the reaction of sodium with chlorine gas according to this equation: Suppose that 6.7 mol of sodium reacts with 3.2 mol chlorine. a. How many moles of sodium chloride are produced? b. What is the limiting reagent? Example Problem: Write the equation for the complete combustion of ethene, C 2 H 4 : If 2.7 mol of ethene is reacted with 6.3 mole of oxygen: a. calculate the moles of water produced b. what is the limiting reagent? 6
7 Example Problem: Write the equation for the incomplete combustion of ethene. If 2.7 mole of ethene is reacted with 6.3 mole of oxygen: a. calculate the moles of water produced b. what is the limiting reagent? Example Problem: When copper reacts with sulfur, solid copper (I) sulfide is produced. Write this combination reaction. a. What is the limiting reagent when 80.0 grams of copper reacts with 25.0 grams of sulfur? b. What is the maximum number of grams of product that can be formed? Example Problem: Hydrogen gas can be produced in the lab by reaction of magnesium metal with hydrochloric acid. Write the COMPLETE balanced equation: a. identify the limiting reagent when 6 grams of HCl reacts with 5 grams of Mg. b. How many grams of hydrogen can be produced? 7
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