Ethylene oxide is produced by reacting ethylene with oxygen. The feed to the reactor contains 5 moles of ethylene, 3 moles of oxygen and 2 moles of ethylene oxide. Set up the compound balances in general and then use these to answer the questions below using the extent of reaction approach. Make sure to interpret the result for each question. 2C,H4 +O2 2C2H¾0 (1) Suppose that ncaH, = 5 mol (i.e., the amount of ethylene coming out of the (a) reactor is 5 moles), how much reaction has occurred? (Ь) Suppose nc,H, = 6 mol, how much reaction has occurred? (c) Suppose nc,H, = 0 mol, how much reaction has occurred? (d) Which component is the limiting reagent, and what is the theoretical yield? (e) Suppose nc,H, = 2 mol, what is the fractional conversion?
Ethylene oxide is produced by reacting ethylene with oxygen. The feed to the reactor contains 5 moles of ethylene, 3 moles of oxygen and 2 moles of ethylene oxide. Set up the compound balances in general and then use these to answer the questions below using the extent of reaction approach. Make sure to interpret the result for each question. 2C,H4 +O2 2C2H¾0 (1) Suppose that ncaH, = 5 mol (i.e., the amount of ethylene coming out of the (a) reactor is 5 moles), how much reaction has occurred? (Ь) Suppose nc,H, = 6 mol, how much reaction has occurred? (c) Suppose nc,H, = 0 mol, how much reaction has occurred? (d) Which component is the limiting reagent, and what is the theoretical yield? (e) Suppose nc,H, = 2 mol, what is the fractional conversion?
Introduction to Chemical Engineering Thermodynamics
8th Edition
ISBN:9781259696527
Author:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart
Publisher:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart
Chapter1: Introduction
Section: Chapter Questions
Problem 1.1P
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![Ethylene oxide is produced by reacting ethylene with oxygen. The feed to the reactor contains 5 moles of ethylene, 3 moles of oxygen, and 2 moles of ethylene oxide. Set up the compound balances in general and then use these to answer the questions below using the extent of reaction approach. Make sure to interpret the result for each question.
\[
2C_2H_4 + O_2 \rightarrow 2C_2H_4O \quad (1)
\]
(a) Suppose that \( n_{C_2H_4} = 5 \) mol (i.e., the amount of ethylene coming out of the reactor is 5 moles), how much reaction has occurred?
(b) Suppose \( n_{C_2H_4} = 6 \) mol, how much reaction has occurred?
(c) Suppose \( n_{C_2H_4} = 0 \) mol, how much reaction has occurred?
(d) Which component is the limiting reagent, and what is the theoretical yield?
(e) Suppose \( n_{C_2H_4} = 2 \) mol, what is the fractional conversion?](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F8dbff956-e43c-48ff-b648-b98fd3ab1747%2F1ec4828f-b56a-4a74-b679-09fde44847bc%2Flwl8xhp_processed.jpeg&w=3840&q=75)
Transcribed Image Text:Ethylene oxide is produced by reacting ethylene with oxygen. The feed to the reactor contains 5 moles of ethylene, 3 moles of oxygen, and 2 moles of ethylene oxide. Set up the compound balances in general and then use these to answer the questions below using the extent of reaction approach. Make sure to interpret the result for each question.
\[
2C_2H_4 + O_2 \rightarrow 2C_2H_4O \quad (1)
\]
(a) Suppose that \( n_{C_2H_4} = 5 \) mol (i.e., the amount of ethylene coming out of the reactor is 5 moles), how much reaction has occurred?
(b) Suppose \( n_{C_2H_4} = 6 \) mol, how much reaction has occurred?
(c) Suppose \( n_{C_2H_4} = 0 \) mol, how much reaction has occurred?
(d) Which component is the limiting reagent, and what is the theoretical yield?
(e) Suppose \( n_{C_2H_4} = 2 \) mol, what is the fractional conversion?
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