Formaldehyde is produced commercially by the catalytic oxidation of methanol. In a side reaction, methanol is oxidized to CO2.
A mixture containing 55.6 mole% methanol and the balance oxygen enters a reactor at 350°C and 1 atm at a rate of 4.60 × 104L/s. The reaction products emerge at the same temperature and pressure at a rate of 6.26 × 104L/s. An analysis of the products yields a molar composition of 36.7% CH2O,4.1% CO2, 14.3% O2. and 44.9% H2O. The required reactor cooling rate is calculated to be 1.05 × 105kW.
- Is the calculated cooling rate correct for the given stream data?
- The stream data cannot be correct. Prove it.
![Check Mark](/static/check-mark.png)
Want to see the full answer?
Check out a sample textbook solution![Blurred answer](/static/blurred-answer.jpg)
Chapter 9 Solutions
EBK ELEMENTARY PRINCIPLES OF CHEMICAL P
Additional Science Textbook Solutions
Elements of Chemical Reaction Engineering (5th Edition) (Prentice Hall International Series in the Physical and Chemical Engineering Sciences)
Process Dynamics and Control, 4e
Java How To Program (Early Objects)
Starting Out with Java: From Control Structures through Objects (6th Edition)
Starting Out with Programming Logic and Design (4th Edition)
Problem Solving with C++ (9th Edition)
- consider the following balancing process at 700c 2H2 (g) + 2s2 (g) 《》 2H2 (g) An analysis shows that there are 2.5 moles of H2, 135 × 10 ^ -5 moles of S2 and 8.70 moles of H2S contained in a 12-liter flask calculating Kc and Kparrow_forward_engine.html?ClassID=D1087757335# Caculate the standard enthalpy for the following reaction conducted at 25°C: MgCl2(s) + 2Na(s) → 2NACI(s) + Mg(s) MgCl2(s) -641.8 kJ/mol NaCl -411.0 kJ/mol AH (kJ/mol) Enterarrow_forwardNIG 2 H₂(g) + O2(g) → 2 H₂O(g) IO AH°--241.8KJ, 促 ASO = -88.85. Assuming AHO=AH and AS-AS, calculate the temperature criterion for spontaneity. Indicate the min. or max temp. required for OROKA spontaneity. T₁S2T=AH HO For this ran, дноarrow_forward
- Consider the balanced reaction 4 A + 4 B → 5C+ 6 D. If 5.577 moles of C (MW = 36.53) are produced, how many grams of A (MW%3D 47.16) are consumed? Report your answer to three decimal places (ignore significant figures).arrow_forward→ C app.101edu.co STARTING AMOUNT esc 1 X 2 F2 CO #m 3 1 The average adult human burns 2.00 × 10³ kcal per day in energy. What is this rate in kJ per hour ? J ADD FACTOR * ( ) X 4184 F4 $ 4 cal 0 349 2.00 × 10³ F5 % 5 kJ Question 26 of 35 O 1000 2.01 x 10⁰ min M 6 31 = 0.001 F7 ANSWER 24 kcal/day O & 7 1.15 x 105 20.0 C F8 S 8 RESET 2 4.184 F9 kcal X 9 F10 60 hr F F11 8 Jan 21 F1Z2 3:17 6 delete Submit + backspacarrow_forwardThe oxidation of ethylene to produce ethylene oxide proceeds according to the equation2C 2H 4 +O 2 ! 2C 2H 4OThe feed to a reactor contains 100 kmol C 2H 4 and 100 kmol O 2. Which reactant is limiting?arrow_forward
- When the following gas reaction reaches equilibrium, at a certain temperature, the moles fractions of the four reactive species satisfy the following relation (we will use "y" for mole fractions since all of these reagents and products are gases): CO+H20 CO2+H2 K= [yCO2][yH2] [yco][yH20] Where K= 1. Assume that the feed introduced to the reactor is 2 mol of CO and 4 mol of H20 only. Also assume that the reaction reaches equilibrium. a) Calculate the extent of reaction in equilibrium (Šeg) b) Calculate the equilibrium composition, for this you need to calculate the mole fraction for all reactants and products.arrow_forwardellus_engine.html?ClassID=1087757335# Calculate the standard reaction enthalpy for the reaction between NO and O3. NO(g) + O3(g) NO2(g) + O2(g) Compound AH°; (kJ/mol) NO(g) 90. AHxn = [ ? ] kJ %3D 0,(8) NO,(g) 143 34 Enter either a + or - sign and the magnitude. Enterarrow_forwardHenry Ford’s Model T was originally designed and built to run on ethanol. Today, ethanol (190-proof alcohol) can be produced with domestic stills for about $0.85 per gallon. When blended with gasoline costing $4.00 per gallon, a 20% ethanol and 80% gasoline mixture costs $3.37 per gallon. Assume fuel consumption at 25 mpg and engine performance in general are not adversely affected with this 20–80 blend (called E20). How much money can be saved for 15,000 miles of driving per year?arrow_forward
- 3. Two moles of an equimolar mixture of CO and H₂O (i.e., one mole of carbon monoxide and one mole of water vapor) is placed in an experimental reactor in which the water- gas shift reaction: CO(g) + H₂O(g) → CO₂(g) + H₂(g) occurs at 2 Atm and at a temperature at which 4G rxn= -0.6932RT. Determine the equilibrium composition (mole fractions) in the reactor.arrow_forward1 mol propane (C3H8) and stoichiometric amount of oxygen (O2) needed to combust propane was preheated to 400 K. After combustion, the products released are at 1500 K. The combustion products are H2O(l) and CO2(g). With 100% conversion was achieved, estimate the total heat released. Calculate the heat requirement for a reactor in combusting 1 mol of methane, CH4, with 25% excess air until the products reach a temperature of 1000 K. The reactants entered the reactor at 298.15 K and 100% conversion of methane is achieved. Assume air is approximately 21% O2 and 79% N2 and products are H2O(l) and CO2(g). Hint for both #1 and #2 – Combustion products at 298 K is CO2(g) and H2O(l). If the exiting temperature is above 373.15 K, H2O will leave as H2O(g). Therefore, you should account for the phase change of H2O(l) to H2O(g).arrow_forward1. Temperature is an intensive property. True or False 2. The value of AH for a given reaction depends on the physical state of each component. True or False 3. In dealing with PV work, the P in PAV always refer to the external pressure- the pressure that causes an expansion. True or False 4. A state function depends on the how the system arrived at the present state. True or False 5. The zero points for AH_f^0 values are elements in their standard state. All substances are measured in relation to this zero point. True or Falsearrow_forward
- ChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage LearningChemistryChemistryISBN:9781259911156Author:Raymond Chang Dr., Jason Overby ProfessorPublisher:McGraw-Hill EducationPrinciples of Instrumental AnalysisChemistryISBN:9781305577213Author:Douglas A. Skoog, F. James Holler, Stanley R. CrouchPublisher:Cengage Learning
- Organic ChemistryChemistryISBN:9780078021558Author:Janice Gorzynski Smith Dr.Publisher:McGraw-Hill EducationChemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage LearningElementary Principles of Chemical Processes, Bind...ChemistryISBN:9781118431221Author:Richard M. Felder, Ronald W. Rousseau, Lisa G. BullardPublisher:WILEY
![Text book image](https://www.bartleby.com/isbn_cover_images/9781305957404/9781305957404_smallCoverImage.gif)
![Text book image](https://www.bartleby.com/isbn_cover_images/9781259911156/9781259911156_smallCoverImage.gif)
![Text book image](https://www.bartleby.com/isbn_cover_images/9781305577213/9781305577213_smallCoverImage.gif)
![Text book image](https://www.bartleby.com/isbn_cover_images/9780078021558/9780078021558_smallCoverImage.gif)
![Text book image](https://www.bartleby.com/isbn_cover_images/9781305079373/9781305079373_smallCoverImage.gif)
![Text book image](https://www.bartleby.com/isbn_cover_images/9781118431221/9781118431221_smallCoverImage.gif)