A mixture of methane, ethane, and argon at 25°C is burned with excess air in a power-plant boiler. The hydrocarbons in the fuel are completely consumed. The following variable definitions will be used throughout this problem:
xm= mole fraction of methane in the fuel
xA= mole fraction of argon in the fuel
Pxs(%) = percent excess air fed to the furnace
Ta(°C) = temperature of the entering air
Ts(°C) = stack gas temperature
r = ratio of CO2to CO in the stack gas (mol CO2/mol CO)
- Without doing any calculations, sketch the shapes of the plots you would expect to obtain for plots of Q versus (i) xM, (ii) xA, (iii) Pxs, (iv) Ta, (v) Ts, and (vi) r, assuming in each case that the other variables are held constant. Briefly state your reasoning for each plot.
- Take a basis of 1.00 mol/s of fuel gas. draw and label a flowchart, and derive expressions for the molar flow' rates of the stack gas components in terms of xM, xA, Pxs, and r. Then take as references the elements at 25°C, prepare and fill in an inlet-outlet enthalpy table for the furnace, and derive expressions for the specific molar enthalpies of the feed and stack gas components in terms of Taand Ts. Calculate
- = -655 kW.) Prepare a spreadsheet that has columns for. xM, xA, P x s , , Ta, r, Ts, and
xM= 0.00—0.85 mol CH4/mol
xA= 0.01—0.05 mol Ar/mol
Pxs= 0%-100%
Ta= 25°C—25O°C
r = 1 — 100 mol CO2/mol CO (make the r axis logarithmic)
Ts= 500°C-1000°C
When generating each plot, use the variable values given in Part (c) as base values. (For example, generate a plot of
![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)
Engineering Mechanics: Statics
Introduction To Finite Element Analysis And Design
Starting Out with C++ from Control Structures to Objects (8th Edition)
- (5) The emissions from a manufacturing process contain gaseous pollutant that cause odors and fumes. The company plans to incinerate the 5,000 acfm exhaust stream. Estimate the volumetric (standard) flowrate of natural gas fuel required to increase the waste gas stream temperature from the initial 80°F to the required temperature of 2500°F. Energy (enthalpy) is transferred from the fuel to the gas. Neglect any possible heat losses in this process. The average net heating value of natural gas is 850 - 1050 Btu/std-ft. Include a diagram of the scenario.arrow_forwardThe specific heat of compound AB(s) was determined using coffee-cup calorimeter. When 1.750 g of AB(s) was mixed with 15.00 mL deionized distilled water at room temperature, only 0.850 grams of the compound was dissolved. The temperature of the heterogenous mixture was decreased by 1.70K.Prior to this, the calorimeter was calibrated using a 15mL aqueous reaction mixture that initially contains 0.070 moles each of HBr and KOH. The recorded ΔT is +5.75K. Note: H+(aq) + OH -(aq) → H2O(l) ΔH = -55.85 kJ/molAB(s) ⇌ A+(aq) + B-(aq) ΔH = 88.75 kJ/molspecific heat (H2O) = 4.184 J/g°CMM of AB = 65 g/mol What is the specific heat of solid AB compound (in J/g°C)?arrow_forwardFive moles of monatomic ideal gas enter the abc cycle and during a complete cycle 600 J of heat is removed from the gas. Process ab is under constant pressure and process bc is increasing at constant volume takes place at pressure. The temperatures of points a and b are Ta-= 3°C and Tb= 63°C. Draw the pV diagram of this cycle.arrow_forward
- Construct enthalpy cycles; use Hess's law and the following data to calculate the enthalpy of formation of ethane (from carbon and hydrogen gas). Cis) + Ozig) + CO2(g) AHa = -394kJmol H2g) + %02(a) – H20 m AH°. = -286kJmol1 + 3%O2(g) → 2002(9) + 3H20 m AH = -1560kJmol1arrow_forwardethylene oxide is prepared by oxidation of ethylene. 100Kmol of ethylene and 100Kmol of O2 are charged to a reactor.The percent conversion of ethylene is 85 and percent yield of C2H4O is 94.12. Calculate the composition of product steam leaving the reactor .The reactions taking place are: C2H4+0.5O2=C2H4O C2H4+3O2= 2CO2+2H2Oarrow_forwardThe growth of the bacterium Zymomonas mobilis in ethanol under aerobic conditions is described by the following global reaction:C2H5OH + a O2 + b NH3 → c C H1.704N0.149O0.408 + d CO2 + e H2Oa) Write the equations for the balance by elements and the balance of electrons.b) determine the coefficients a, b, c, and d knowing that RQ = 0.66c) determine YX/S and YX/O2arrow_forward
- What is the standard enthalpy of reaction per mole of either HCl or NaOH when 50.00 cm3 of 0.1 moldm-3 of hydrochloric acid (HCl) and 50.00 cm3 of 0.1 moldm-3 of sodium hydroxide (NaOH) are mixed? According to your simulation, the temperature rose by ___0.68__ oC. (Density of water = 1gcm-3, Specific heat capacity of water = 4.18 J g-1 oC-1) Show your working below: HCl (aq) + NaOH(aq) à NaCl(aq) + H2O(l)arrow_forwardA gaseous fuel containing methane and ethane is burned with excess air. The fuel enters the furnace at 25°C and 1 atm, and the air enters at 200°C and 1 atm. The stack gas leaves the furnace at 800°C and 1 atm and contains 5.32 mole% CO2, 1.60% CO, 7.32% O₂, 12.24% H₂O, and the balance ₂. 1. Calculate the molar percentages of methane and ethane in the fuel gas and the percentage excess air fed to the reactor. 2. Calculate the heat (kJ) transferred from the reactor per cubic meter of fuel gas fed. 3. A proposal has been made to lower the feed rate of air to the furnace. State advantages and a drawback of doing so.arrow_forwardConstruct enthalpy cycles; use Hess's law and the enthalpy changes of formation below to calculate the enthalpy change for the reaction, CaCos(s) – ÇaQ(s) + CO2(g) AH, Cacoa(s) = -1207 kJmol-1 AH Cao(s) = -635 kJmol AH CO2(9) = -393 kJmol 1arrow_forward
- The production of cement results in significant GHG emissions. The emissions are caused by the decomposition of calcium carbonate (limestone) to calcium oxide (lime) and carbon dioxide. This process known as calcination, is carried out in kilns. Therefore, additional GHGs are emitted as a result of heating the kilns. A large cement manufacturer uses a mix of coal, natural gas, and biomass in its boiler. This mix produces the following amounts of GHGs per Million BTUs of energy: • 250 lbs CO2/MMBtu • 5 lbs CH4/MMBtu • 0.36 lbs N2O/MMBtu Process carbon emissions from the calcination process produce 925 lbs of carbon dioxide per metric ton of cement. In addition, the plant uses 1.7 Million BTUs of energy per metric ton of cement. If the plant produces 180,000 metric tons of cement annually, how many metric tons of CO2e does it emit?arrow_forwardIn a generic chemical reaction involving reactants and B and products C and D, aA + bB cC + dD, the standard enthalpy AHin of the reaction is given by AHixn = CAH; (C) + dAH; (D) —aAH (A) – bAH (B) Notice that the stoichiometric coefficients, a, b, c, d, are an important part of this equation. This formula is often generalized as follows, where the first sum on the right-hand side of the equation is a sum over the products and the second sum is over the reactants: where m and n represent the appropriate stoichiometric coefficients for each substance. Part A What is AHxn for the following chemical reaction? CS2(g) + 2H₂O(1)→CO2(g) + 2H₂S(g) You can use the following table of standard heats of formation (AH) to calculate the enthalpy of the given reaction. ■ μÅ Value AHrxn=products H - Σreactants mΔΗ Element/ Compound H(g) H₂(g) H₂O(1) CS2 (g) C(g) C(s) Units ? Standard Heat of Formation (kJ/mol) Express the standard enthalpy of reaction to three significant figures and include the…arrow_forwardThe synthesis of methanol from carbon monoxide and hydrogen is carried out in a continuous vapor-phase reactor at 5.00 atm absolute. The feed contains cO and H2 in stoichiometric proportion and enters the reactor at 25.0°C and 5.00 atm at a rate of 31.1 m³/h. The product stream emerges from the reactor at 157°C. The rate of heat transfer from the reactor is 21.0 kW. Calculate the fractional conversion (0 to 1) of carbon monoxide achieved and the volumetric flow rate (m3/h) of the product stream. f = Vout ! m3/harrow_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)