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: McGraw-Hill Education
expand_more
expand_more
format_list_bulleted
Related questions
Concept explainers
Question
C2H6(g) ---> C2H4(g) + H2(g)
this is the reaction.....please do problem 5 i have added problem 4 because it is brought up in problem 5
![**Transcription for Educational Website**
---
4. Consider the production of ethylene from the decomposition of ethane as shown in the following reaction:
\[ \text{C}_2\text{H}_6 \, (\text{g}) \rightleftharpoons \text{C}_2\text{H}_4 \, (\text{g}) + \text{H}_2 \, (\text{g}) \]
What is the maximum possible conversion at a temperature of 1000º C and a pressure of 1 bar? Assume \(\Delta H^\circ_{\text{rxn}}\) to be constant.
---
(Includes no graphs or diagrams)](https://content.bartleby.com/qna-images/question/c2a758a4-69fc-4b07-9ca9-f4af1d363e17/2be0ddc0-631e-4784-bfc5-dd3f2c44cff7/y9izwdn_processed.png)
Transcribed Image Text:**Transcription for Educational Website**
---
4. Consider the production of ethylene from the decomposition of ethane as shown in the following reaction:
\[ \text{C}_2\text{H}_6 \, (\text{g}) \rightleftharpoons \text{C}_2\text{H}_4 \, (\text{g}) + \text{H}_2 \, (\text{g}) \]
What is the maximum possible conversion at a temperature of 1000º C and a pressure of 1 bar? Assume \(\Delta H^\circ_{\text{rxn}}\) to be constant.
---
(Includes no graphs or diagrams)
Transcribed Image Text:5. For the reaction in problem 4 above, which of the following conditions would you use? Explain.
a) 600 ºC and 1 bar.
b) 1500 ºC and 1 bar.
c) 1500 ºC and 75 bar.
(You do not need to make calculations, using the governing equations and Le Chatelier’s principle, explain clearly and briefly)
Expert Solution
This question has been solved!
Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.
Step by stepSolved in 2 steps
Knowledge Booster
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemical-engineering and related others by exploring similar questions and additional content below.Similar questions
- What kind of reaction mechanism would allow for the below reaction? Select one or more: a. El O b. SN2 □ ☐ c. E2 d. SN1 Θ 4arrow_forwardThe reaction of CO(g) with NO2 (9) is second-order in NO2 and zero-order in CO at temperatures less than 500 K. a. Write the rate law for the reaction. (Rate expressions take the general form: rate = k[H2][C12].) rate b. How will the reaction rate change if the NO2 concentration is tripled? The reaction rate will be the original value. c. How will the reaction rate change if the concentration of CO is tripled? The reaction rate will be the original value.arrow_forward1. Consider the following unbalanced reaction, Cl2(g) + NO(g) ---> NOCl(g) a). Suppose that 150.0 g of NO is allowed to react with 220.0 g of Cl2. What is the largest amount of NOCl that could be formed in this reaction? b) What was the yield if only 31.5 g was actually formed? (corresponds to part a) 2.Draw a diagram of y against r for a 3s. What 2 features does it imply that do not make much sense? How can these problems be avoided? Give and explanation and diagrams/graphsarrow_forward
- An engineer wants to look into the kinetics of the degradation of atrazine (A). There are 2 ways for degradation to occur. First, dealkylation to develop deisopropylatrazine (B) and deethylatrazine (C) with a kinetic constant of k1. Second, hydrolysis to create hydroxyatrazine (D) and N-isopropylammelide (E) with a kinetic constant k2. For all the mentioned species, derive their concentration profiles as a function of time when a batch reactor is utilized.arrow_forwardReaction engineering Please derive the rate law equation (rp ) for the following enzymatic reaction with with inhibition from the product P E+S <-------> E*S (k1 in the foward direction and k2 backwards) E*S -----------> E+P (k3) E+P <-------> E*P (k4 in the foward direction and k5 backwards )arrow_forwardUsing Le Chatilier's Pronciple to predict whether adding some HClO (aq) causes the system to shift in the direction to products or reactions: HClO + H20= H20+ ClOarrow_forward
- Calculate the reaction enthalpy for the reaction below: 2 C(s) + D (g) →→→2 A (s) +2B (s) given the following information X (s) + D (g) →→→ A (s) Y(g) +B(s)→→→ Z (g) X (s) +Z (g) →→→ C(s) +Y(g) AH, : AH, = ? kJ AH₁ = -263.0 kJ AH₂ = -75.0 kJ AH3 = -455.0 kJ kJarrow_forwardI want you to give me step by step solution and describe everything.arrow_forwardThe reaction below was determined experimentally to be first order in both NO2 and O3: 2NO2(g) + O3(g) → N2O5(g) + O2(g) Which proposed mechanism(s) is/are consistent with the observed rate law? Mechanism I: O3 40 + O2 O + NO2 → NO3 NO2 + NO3 → N2O5 Step 1 (fast, equilibrium) Step 2 (slow) Step 3 (fast) Mechanism II: Step 1 O3 + NO2 NO3 + O2 slow Step 2 NO2 + NO3 → N2O5 fast Neither I and II Il only O I only Both I and IIarrow_forward
- Using the graphic below as a reference, describe what happens to a reversible reaction as it attains equilibrium.arrow_forwardConsider the following mechanisms for the Hydrogen Evolution Reaction: Mechanism 2 Mechanism 1 H(aq) Haq) + e- H2(g) 2 H (ads) H2(g) H(ads) + H(aq) + e Describe, in detail, how one could differentiate between these mechanisms experimentally. +e¯ H(ads) H(ads) -arrow_forwardWhich of the following is NOT required for a reaction to occur? The reactants must collide with the correct orientation. All are required for a reaction to occur. The reactants must surpass the activation energy required for the reaction. The bonds of the products must formed. The reactants must collide with each other with sufficient energy to break bonds and form the activated complex.arrow_forward
arrow_back_ios
SEE MORE QUESTIONS
arrow_forward_ios
Recommended textbooks for you
- Introduction to Chemical Engineering Thermodynami...Chemical EngineeringISBN:9781259696527Author:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark SwihartPublisher:McGraw-Hill Education
Elementary Principles of Chemical Processes, Bind...Chemical EngineeringISBN:9781118431221Author:Richard M. Felder, Ronald W. Rousseau, Lisa G. BullardPublisher:WILEY
Elements of Chemical Reaction Engineering (5th Ed...Chemical EngineeringISBN:9780133887518Author:H. Scott FoglerPublisher:Prentice Hall 
Industrial Plastics: Theory and ApplicationsChemical EngineeringISBN:9781285061238Author:Lokensgard, ErikPublisher:Delmar Cengage Learning
Unit Operations of Chemical EngineeringChemical EngineeringISBN:9780072848236Author:Warren McCabe, Julian C. Smith, Peter HarriottPublisher:McGraw-Hill Companies, The
Introduction to Chemical Engineering Thermodynami...
Chemical Engineering
ISBN:9781259696527
Author:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart
Publisher:McGraw-Hill Education
Elementary Principles of Chemical Processes, Bind...
Chemical Engineering
ISBN:9781118431221
Author:Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:WILEY
Elements of Chemical Reaction Engineering (5th Ed...
Chemical Engineering
ISBN:9780133887518
Author:H. Scott Fogler
Publisher:Prentice Hall
Industrial Plastics: Theory and Applications
Chemical Engineering
ISBN:9781285061238
Author:Lokensgard, Erik
Publisher:Delmar Cengage Learning
Unit Operations of Chemical Engineering
Chemical Engineering
ISBN:9780072848236
Author:Warren McCabe, Julian C. Smith, Peter Harriott
Publisher:McGraw-Hill Companies, The