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Chapter 3 Limiting Reactants

Chapter 3 Limiting Reactants - 1 Fe 2 O 3 2Fe 2 Theoretical...

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Eugene Kim General Chemistry: Chapter 3 – Limiting Reactants September 17, 2009 I) Reaction Yield a. Assumption that reaction goes to completion and that only the products written are formed i. Sometimes unwanted “by-products” (side reactions) also occur ii. Products (or reactants) can be lost before they are used or measured b. Theoretical Yield i. The amount of product that should be produced ideally II) % Yield a. Amount of product that is really produced is called the actual yield i. Cannot be predicted, but must be measured b. % Yield = (actual yield / theoretical yield) x 100% i. Is like testing for error percentage c. Example i. 15 kg of Fe 2 O 3 is reduced to Fe. 8.8 kg are produced. What is the percent yield?
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Unformatted text preview: 1. Fe 2 O 3 2Fe 2. Theoretical Yield a. 10.49 kg 3. Percent Yield a. 8.8/10.5 = 83.9% III) Lim iting Reactants a. Identifying the Lim iting Reactants i. Step 1: Balance the equation ii. Step 2: Find the number of moles of each reactant present iii. Step 3: Determine the number of moles of each reactant needed to completely use one reactant 1. You will either have more than enough of the other reactant or one or more reactants will not be present in large enough amounts 2. The compound which is “short” by the largest amount is the lim iting reactant b. Example i. 100 g of CaC 2 is mixed with 100 g of water. Which is the limiting reactant?...
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