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2. Pentane combusts with oxygen to form carbon dioxide and water by the following reaction: C5H12(1) +8 O2(g) → 5 CO2(g) + 6 H₂O(g) a. If 0.111 moles of pentane (CsH12) is mixed with 0.313 moles of oxygen (O₂), which is the limiting reactant?

2. Pentane combusts with oxygen to form carbon dioxide and water by the following reaction: C5H12(1) +8 O2(g) → 5 CO2(g) + 6 H₂O(g) a. If 0.111 moles of pentane (CsH12) is mixed with 0.313 moles of oxygen (O₂), which is the limiting reactant?

Chemistry: The Molecular Science
Chemistry: The Molecular Science
5th Edition
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter3: Chemical Reactions
Section: Chapter Questions
Problem 110QRT
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Limiting Reactant, Theoretical Yield and Percent Yield 2. Pentane combusts with oxygen to form carbon dioxide and water by the following reaction: C5H12(l) +8 O2(g) → 5 CO2(g) + 6 H₂O(g) a. If 0.111 moles of pentane (C5H12) is mixed with 0.313 moles of oxygen (O₂), which is the limiting reactant? 28 < 6 C 17 > O 6
Transcribed Image Text:Limiting Reactant, Theoretical Yield and Percent Yield 2. Pentane combusts with oxygen to form carbon dioxide and water by the following reaction: C5H12(l) +8 O2(g) → 5 CO2(g) + 6 H₂O(g) a. If 0.111 moles of pentane (C5H12) is mixed with 0.313 moles of oxygen (O₂), which is the limiting reactant? 28 < 6 C 17 > O 6
b. What is the theoretical yield (in grams) of carbon dioxide and water for this reaction? 3. Hydrogen reacts with nitrogen to form ammonia by the following equation: 3 H₂(g) + N2(g) → 2 NH3(g) a. What is the limiting reactant if 1.60 g of hydrogen are mixed with 6.90 g of nitrogen? b. What is the theoretical yield of ammonia (in grams)? c. Calculate the percent yield of ammonia when 7.45 grams of ammonia was experimentally obtained from the reaction? S
Transcribed Image Text:b. What is the theoretical yield (in grams) of carbon dioxide and water for this reaction? 3. Hydrogen reacts with nitrogen to form ammonia by the following equation: 3 H₂(g) + N2(g) → 2 NH3(g) a. What is the limiting reactant if 1.60 g of hydrogen are mixed with 6.90 g of nitrogen? b. What is the theoretical yield of ammonia (in grams)? c. Calculate the percent yield of ammonia when 7.45 grams of ammonia was experimentally obtained from the reaction? S
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