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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(1)+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 (0₂), which is the limiting reactant?

Limiting Reactant, Theoretical Yield and Percent Yield 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 (C5H12) is mixed with 0.313 moles of oxygen (0₂), which is the limiting reactant?

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Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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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(1) +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? O 6 /7 > ||| HA
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(1) +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? O 6 /7 > ||| HA
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? < 7/2> 111
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? < 7/2> 111
Expert Solution
Step 1: Combustion reaction

2.

The given combustion reaction is C5H12(l) + 8O2(g) rightwards arrow 5CO2(g) + 6H2O(g).

Given that, 0.111 moles of pentane is mixed with o.313 moles of oxygen.

We have to detect the limiting reactant and the theoretical yield of the carbon dioxide and water.


Limiting reactant: In a reaction, the substance which is present in lesser amount is called the limiting reactant.

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