Adipic acid, \(\mathrm{H}_{2} \mathrm{C}_{6} \mathrm{H}_{8} \mathrm{O}_{4}\), is used to produce nylon, The acid is made commercially by a controlled reaction between cyclohexane \(\left(\mathrm{C}_{6} \mathrm{H}_{12}\right)\) and \(\mathrm{O}_{2}\):

\(2\mathrm{\ C}_6\mathrm{H}_{12}(l)+5\mathrm{\ O}_2(g)\rightarrow2\ \mathrm{H}_2\mathrm{C}_6\mathrm{H}_8\mathrm{O}_4(l)+2\mathrm{\ H}_2\mathrm{O}(g)\)

(a) Assume that you carry out this reaction with 25.0 g of cyclohexane and that cyclohexane is the limiting reactant. What is the theoretical yield of adipic acid?

(b) If you obtain 33.5 g of adipic acid from your reaction, what is the percent yield of adipic acid?

Solution

Step 1 of 2

(a) The theoretical yield is:

\(=(125.0\ g\ C_6H_{12})\times(1\ mol\ C_6H_{12})\times(2\ mol\ H_2C_6H_8O_4)(2\ mol\ C_6H_{12})\times(146.0\ g\ H_2C_6H_8O_4)(1\ mol\ H_2C_6H_8O_4)\)

\(=43.4\ g\ H_2C_6H_8O_4\)

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Title Chemistry: The Central Science 13

Author Theodore E. Brown; H. Eugene LeMay; Bruce E. Bursten; Catherine Murphy; Patrick Woodward; Matthew E. Stoltzfus

ISBN 9780321910417

Solved: Calculating Theoretical Yield and Percent

Chapter 3.20SE textbook questions

Chapter : Problem 1 Chemistry: The Central Science 13
Problem 1PE Calculating Theoretical Yield and Percent Yield Adipic acid, H2C6H8O4, used to produce nylon, is made commercially by a reaction between cyclohexane (C6H12) and 02: 2 C6H12(/) + 5 02(g)—>2 H2C6H8O4(/) + 2 H2O(g) (a) Assume that you carry out this reaction with 25.0 g of cyclohexane and that cyclohexane is the limiting reactant. What is the theoretical yield of adipic acid? (b) If you obtain 33.5 g of adipic acid, what is the percent yield for the reaction? If 3.00 g of titanium metal is reacted with 6.00 g of chlorine gas, CI2, to form 7.7 g of titanium (IV) chloride in a combination reaction, what is the percent yield of the product? (a) 65%, (b) 96%, (c) 48%, or (d) 86%.
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Chapter : Problem 2 Chemistry: The Central Science 13
Calculating Theoretical Yield and Percent Yield Adipic acid, \(\mathrm{H}_{2} \mathrm{C}_{6} \mathrm{H}_{8} \mathrm{O}_{4}\), used to produce nylon, is made commercially by a reaction between cyclohexane \(\left(\mathrm{C}_{6} \mathrm{H}_{12}\right)\) and \(\mathrm{O}_{2}\): \(2\ \mathrm{C}_{6} \mathrm{H}_{12}(l)+5\ \mathrm{O}_{2}(g) \longrightarrow 2\ \mathrm{H}_{2} \mathrm{C}_{6} \mathrm{H}_{8} \mathrm{O}_{4}(l)+2\ \mathrm{H}_{2} \mathrm{O}(g)\) (a) Assume that you carry out this reaction with of cyclohexane and that cyclohexane is the limiting reactant. What is the theoretical yield of adipic acid? (b) If you obtain 33.5 g of adipic acid, what is the percent yield for the reaction? Imagine you are working on ways to improve the process by which iron ore containing \(\mathrm{Fe}_{2} \mathrm{O}_{3}\) is converted into iron: \(\mathrm{Fe}_{2} \mathrm{O}_{3}(s)+3 \mathrm{CO}(g) \longrightarrow 2 \mathrm{Fe}(s)+3 \mathrm{CO}_{2}(g)\) (a) If you start with of \(\mathrm{Fe}_{2} \mathrm{O}_{3}\) as the limiting reactant, what is the theoretical yield of Fe? (b) If your actual yield is , what is the percent yield? Equation Transcription: Text Transcription: Equation Transcription: H_{2}C_{6}H_{8}O_4 (C_{6}H_{12}) O_2 2 C_{6}H_{12}(l)+5 O2(g){rightarrow}2 H2C6H8O4(l)+2 H_{2}O(g) Fe_{2}O_{3} Fe_{2}O_{3}(s)+3 CO(g){rightarrow}2 Fe(s)+3 CO_{2}(g) Fe_{2}O_{3} Fe
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Chapter 3.20SE textbook questions

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Textbook Solutions for Chemistry: The Central Science

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