Ethylene gas and steam at atmospheric pressure are fed to a reaction process as an equimolarmixture. The process produces ethanol by the reaction:C₂H₂(g) +H₂O(g)→C,H,OH (1)The liquid exits the process at 25°C. An amount of 120,000 J heat per mole of ethanol is producedby the process. Calculate the temperature of feed to the process?Information: Heat of reactions at 25°C and mean heat capacity at ideal gas state are available as inTable Q4.Table Q4. The value of R = 8.314 J/mol.KCompoundC₂H4 (g)H₂O(g)C₂H5OH (1)AH 298 (J/mol)52510-241818-277690(CIR744

Given reaction of ethylene and steam is C2H4(g)+H2O(g)→C2H5OH(l) Also given data are as follows:…

Answered: Ethylene gas and steam at atmospheric…

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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An equimolar mixture of nitrogen and acetylene enters a steady-flow reactor at 25°C and atmospheric pressure. The only reaction occurring is: N2(g) + C2H2 → 2HCN(g)N2(g) + C2H2 → 2HCN(g) The product gases leave the reactor at 600°C and contain 24.2 mol-% HCN. How much heat is supplied to the reactor per mole of product gas? (Use the tables for standard enthalpies and gibbs energies of formation and the heat capacities of gases in the ideal gas state.)
P6.36 We need to calculate a standard-state AĦ", for the oxidation of p-xylene (CH1,) to terephthalic acid (TPA, C,O̟H), which is used in making plastic 2-L soda bottles. However, heats of formation of the compounds from the respective elements are not available. Reference tables do have information on heats for combustion to CO, (g) and H,O (1) at 25°C, and show that the energy released is 1089 kcal/mol for p-xylene (1) and 770 kcal/mol for TPA (s). C,H1, (1) + 3 O, (g) → C,0̟H, (s) +2 H,0 (1) -94 Determine a numerical value for AÊĤº. Given that AĤĦ; for CO2 kcal/mol and AĤ, for liquid H,O p-xylene and TPA. = -68 kcal/mol, calculate AH for
9.20. Ammonia is oxidized with air to form nitric oxide in the first step of the production of nitric acid. Two principal reactions occur: 4 NH3 + 5 024 NO + 6 H₂O 2 NH3 + 2O₂ → N₂ + 3 H₂O A flowchart of the reactor follows. 100 mol NH3(g)/min 25°C, 8 bar 900 mol air/min 0.21 02 0.79 N₂ 150°C, 8 bar REACTOR Product gas: 700°C, 8 bar 90 mol NO/min 0000 150 mol H₂O(v)/min 716 mol N₂/min 69 mol 0₂/min ġ(kJ/min)
Exercise 7.2.1: Heat from a generic reaction. A balance stoichiometric reaction 2D + 0.5E 3.8F with Ah-(100°C, 1 atm) = -48 kJ/mol. (a) If 62 mol/s of component F are produced at 100°C and 1 atm, how much heat (kW) is produced by the reaction?
The heat of combustion of undecane is - 7430.9 kJ/mol. Use this value to find the heat of formation of undecane. (You may also need to use the following tabulated thermochemical data. Enter an unrounded value.) Substance AH° (kJ mol-) 02 (9) CO2 (9) -393.5 H, O(1) -285.8 C; H12 (1) -173.5 C,H16 (1) -224.2 C9 H20 (1) -274.7 C11H24 (1) -327.2 kJ/mol Activate Windows
Determine the specific volume of refrigerant-134a at 2MPA and 100°C, using (a). the ideal-gas equation of state.---- (b). the Vander Waals EOS. (Calculate the Vander Waals EOS parameters using the equations and obtain the data values form the steam tables).Compare the values obtained to the experimentally determined value of 15,000 KPa.---- (c).Using the generalized compressibility chart. Determine the error involved in each case.----
The heat capacities for each of the substances involved for a particular reaction are given below. The enthalpy change for the same reaction at 298 Kelvin is -282.987 KJ/mole. From these, answer the questions that follow. Temperature-Dependence of the heat capacities of the Substances for the given reaction + (1/2)02(9) → CO2(9) For the gaseous reaction; CO the heat capacities are: Cp°co P(g) 26.86 + 6.97 x10-3 T - 8.20 x10-7 T2 %3D Cp°o2 25.72 + 12.98 x10-3 T - 38.60 x10-7 T² %3D Cp°co2 26.00 + 43.50 x10-3 T 148.32 x10-7 T² %3D What would be the overall enthalpy change at 1,000 Kelvin (AH @ 1000K, in KJ)?
At approximately atmospheric pressure, methane gas is burned completely with 30% excess air. Both the air and methane enter the furnace at 30 °C saturated with water vapor, and the flue gases leave the furnace at 1500 °C. Calculate how much heat is lost from the furnace per mole of methane. In your solution, show analytically all calculations, including the analytical derivation of the number of moles of water vapor entering the furnace. Use steam tables to determine Psat, and compare your answer with the answer you would obtain using Antoine’s and Wagner’s equations. For the latter, you can determine A, B, C, D as in ** above.
. CO₂ entering from a combustion (T = 500°C) process is mixed stoichiometrically with H₂ at (T= 25°C). A reaction occurs over a catalyst producing water and methane with a 70% conversion of the reactants. If the products leaving the reactor have a temperature of 725°C calculate the heat transfer to or from the reactor. CO₂ + 4H₂ → 2H₂O+CHA Assume Constant Cp for all components except H₂O. kJ mole. C CO2: Cp= 0.037 kJ mole C CO₂ T = 500°C H₂ T = 25°C H2: Cp = 0.029. Reactor kJ mole. C CH4: Cp = 0.033- CO2, H2, H₂O, CH4 T = 725°C

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