What does this equation tell you? 1. 1 molecule of nitrogen gas reacts with 3 molecules of hydrogen gas to produce 2 molecules of ammonia gas.

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1 Chapter 7 Quantities in Chemical Reactions Stoichiometry For example, the Haber Process (used to make ammonia gas) is based on the following balanced equation: N 2(g) + 3H 2(g) 2NH 3(g) Stoichiometry is the study of the relative quantities of reactants and products in chemical reactions. It all begins with balanced chemical equations, which are essential for making calculations related to chemical reactions. What does this equation tell you? 1. 1 molecule of nitrogen gas reacts with 3 molecules of hydrogen gas to produce 2 molecules of ammonia gas. If we multiply each by 12 we could say: 1 dozen molecules of nitrogen gas reacts with 3 dozen molecules of hydrogen gas to produce 2 dozen molecules of ammonia gas. 2. If we wanted 100 molecules of ammonia gas, we would need 50 molecules of nitrogen gas and 150 molecules of hydrogen gas because the ratio is 1:3:2

2 4. If we multiply each by 6.02x10 23 we could say: 1 mole of nitrogen gas reacts with 3 moles of hydrogen gas to produce 2 moles of ammonia gas. The relationship between moles in a balanced chemical equation are known as MOLE RATIOS We use mole ratios to solve problems. 1. From the equation above, how much ammonia gas would be produced from 3.5 mol of hydrogen gas? 2. When carbon and oxygen combine 2 reactions are possible. The product can be CO 2 or CO. a. Write the balanced chemical equations. b. How much oxygen is needed to react with 0.75mol carbon to produce CO 2? c. How much oxygen is needed to react with 0.75mol carbon to produce CO?

3 Mole Ratios can also be used to find the mass ratios for chemical equations. N 2(g) + 3H 2(g) 2NH 3(g) If you know the amount of one substance in a chemical reaction (moles, particles, mass) you can calculate the amount of any other substances in the reaction using the BALANCED CHEMICAL EQUATION. Solving Stoichiometric Problems Follow this process: 1. Write a balanced equation. 2. If you are given the mass or # of particles of a substance, convert it to the # of moles. 3. Calculate the # of moles of the required substance based on the # of moles of the given substance, using mole ratios. 4. Convert the # of moles of the required substance to mass or # of particles. Ex 1. Mass to Mass Astronauts must be able to remove the CO 2 from their spacecraft. If not hypoxia (lack of O 2 ) would occur. CO 2 is removed using the following chemical reaction: CO 2(g) + 2LiOH (s) Li 2 CO 3(g) + H 2 O (g). If an astronaut produces 1.50x10 3 g of CO 2 a day, what mass of LiOH would be needed per day?

4 Ex 2. On Feb, 20, 2008 the US Navy shot down a spy satellite in space from a war ship in the Pacific ocean. They claimed the satellite contained hydrazine (rocket fuel), that could harm people if the satellite fell back to Earth. When hydrazine is combined with dinitrogen tetroxide it produces nitrogen gas and water. If 100g of hydrazine (N 2 H 4 ) is reacted, how much nitrogen gas would be produced? Ex 3. During WWI, chlorine gas was used as a weapon. When chlorine gas enters the lungs it reacts with water and forms corrosive hydrochloric acid and oxygen gas. How many molecules of chlorine react to produce 5.0g of HCl? Magnesium reacts with cuprous chloride in a single displacement reaction. How much magnesium is required to produce 200g of copper? The Limiting Reactant Chemical reaction equations give the ideal stoichiometric relationship among reactants and products. However, the reactants for a reaction in an experiment are not necessarily a stoichiometric mixture. What mass of cuprous chloride is needed?

5 In a chemical reaction, one of the reactants may not be used up when the reaction is finished. These are called excess reagents. The reagent that is completely used up or reacted is called the limiting reagent, because its quantity limit the amount of products formed. Think of when you put gas in your car: 2C 8 H O 2 16CO H 2 O Ideally, 25 moles of oxygen react with 2 moles of octane. But in reality O 2 is UNLIMITED in the air so octane would be the limiting reactant. When you run out of gas the reaction STOPS! In stoichiometric problems: IF YOU ARE GIVEN THE AMOUNTS OF 2 OR MORE REACTANTS, YOU MUST FIRST IDENTIFY THE LIMITING REACTANT!

6 Ex 1. Glucose reacts with oxygen gas to produce carbon dioxide and water during cellular respiration. If 1.25 g of glucose reacts with 7.51g of oxygen gas, find the limiting reactant. Warmup: 30g of aluminum oxide and 20g of water react to form aluminum hydroxide. What is the limiting reactant? Ex 2. A 2.00g piece of phosphorus is burned in a flask containing 6.91 g of oxygen gas. What mass of tetraphosphorus decaoxide is produced? Iron and carbon dioxide can be produced when iron(iii) oxide reacts with carbon monoxide gas. If 11.5 g of of iron(iii) oxide is reacted with 2.63x10 24 molecules of carbon monoxide, what mass of iron is expected?

7 Percentage Yield Chemists use stoichiometry to predict the amount of a product that can be expected from a chemical reaction. This amount is called the THEORETICAL YIELD. This amount is not always obtained. The actual amount obtained in an experiment is called the ACTUAL YIELD. The actual yield is usually less then the theoretical yield and for a variety of reasons. For example: a. Less than perfect collection techniques b. Competing reactions c. Poor experimental design d. Impure reactants % Yield = Actual Yield x100% Theoretical Yield Ex1. When 75g of nitrogen gas reacts with sufficient hydrogen gas, the theoretical yield of ammonia is 9.10 g. If 1.72 g of ammonia is obtained what is the percentage yield? PERCENTAGE YIELD compares the mass of product obtained by experiment (actual) to the mass predicted by stoichiometry (theoretical).

8 Ex 2. When Calcium carbonate is decomposed to calcium oxide and carbon dioxide there is a 92.4% yield of calcium oxide. How many grams of calcium oxide can you expect if 12.4 g of calcium carbonate is heated. % Purity is the percent of a specific compound in an impure substance.

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