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Limiting Reactants and Percent Yields - video -solutions

# Limiting Reactants and Percent Yields - video -solutions -...

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nanni (arn437) – Limiting Reactants and Percent Yields - video – CNS – (87654) 1 This print-out should have 2 questions. Multiple-choice questions may continue on the next column or page – find all choices before answering. 001 10.0points If a reaction of 5.0 g of hydrogen with 5.0 g of carbon monoxide produced 4.5 g of methanol ? H 2 + ? CO ? CH 3 OH what was the percent yield? 1. 79% correct 2. 28% 3. 37% 4. 66% 5. 13% Explanation: Experimental yield = 4.5 g This question comprises both the limiting reactant and percent yield concepts. % yield = experimental yield theoretical yield × 100% Balance the chemical equation: 2 H 2 + CO 2 -→ CH 3 OH (4 . 04 g) (28 . 01 g) (32 . 05 g) Determine the limiting reactant: The required ratio is 28 . 01 g CO 4 . 04 g H 2 = 6 . 93 g CO g H 2 and the ratio of the masses is 5 . 0 g CO 5 . 0 g H 2 = 1 . 0 CO g H 2 so CO is limiting. Determine the theoretical yield of the reac- tion based on the limiting reactant: (5 g CO) parenleftbigg 32 . 05 g CH 3 OH 28 . 01 g CO parenrightbigg = 5 . 7 CH 3 OH Determine the percent yield: % yield = experimental yield

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