RefExample 9.5-3: The dehydrogenation of ethanol to form acetaldehyde is carried out in acontinuous adiabatic reactor. Ethanol vapor is fed to the reactor at 400 °C, and a conversion of30% is obtained. Calculate the product Temperature.CpSisto 48 có xio7+2.38 X10 T05 x 10-872C₂H5OH(v)→ CH3CHO(v) + H₂(g)SolutionREACTOR100 mol C₂H5OH(v)400°CC₂H50H (V), CH³ CHO (V), H₂a70 mol C₂H5OH(v)30 mol CH3CHO(v)30 mol H₂(g)Tad (°C)

Given reaction is- C2H5OH(v)→CH3CHO (v)+ H2(g) Basis feed of ethanol, C2H5OH= 100 mol Feed…

Answered: Example 9.5-3: The dehydrogenation of…

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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Benzene vapor is burned in air. Find the molar enthalpy of the reactants and the products if all heat is extracted from the reaction and the initial and final temperatures are equal. (Assume the H2O product is a liquid)
The equilibrium constant with respect to temperature can be expressed for the reaction: Cyclohexane (g)! <--> methylcyclopentane (g) as: LnK = 4.814-2059/T. If placed to react 3 moles cyclohexane in a 5 liter container at a certain temperature and when equilibrium is reached, 8000 J of heat is released, Calculate the temperature of the container.
Alumina from bauxite separation stage calculations A crucial step in the production of aluminum from bauxite ore is the separation of alumina from the remaining mineral impurities in the ore. In the Bayer process this is accomplished by treating bauxite with aqueous NaOH to produce NaAIO2 (alumina). NaOH(aq) + Al(OH)3(s) → NaAIO2(aq) + 2H2O(1) Since NaAIO2 is water soluble while the residual mineral constituents of bauxite are not, a separation can be achieved by allowing the minerals to settle out and decanting the aqueous solution of NAAIO2 and unreacted NaOH. In order to further recover any NAAIO2 entrained in the settled mineral solids, this "mud" is repeatedly washed with water and allowed to settle, and the wash water is decanted. The figure below shows one stage of this washing-settling process. Wash water Slurry - Open to air Mixer/Wash tank Setling tank Decanted solution System boundary Washed mud In this stage, a feed slurry consisting of 10 wt% solids, 11 wt% NaOH, 16 wt%…
Ammonia is produced by the catalytic reaction of nitrogen and hydrogen.a) Write the chemical reaction and balance it. Determine the stoichiometric coefficients.b) If 15 mol/sec of H2 is fed to the reactor, determine the amount of N2 required if a 20.%excess (of N2) is desired.c) If 5.0 mol/sec of H2 exits the catalytic reactor, determine: - the number of moles of all three components exiting the reactor. - the conversion of H2 and N2. -the exiting concentration of H2, N2, and ammonia.d) What are strategies to increase the conversion of H2?
One of the ways that benzene is produced on a large scale is the hydrodealkylation of toluene. C,H,CH; + H, C,H, + CH4 A stream of toluene is mixed with a recycle stream and enters a reactor along with a stream of pure hydrogen. The reaction products at 550 °C enter a condenser, where they are cooled to 41.0 °C. A vapor stream containing Y5CH, = 0.600 mol CH,/mol leaves the process, and a liquid stream containing x66 = 0.810 mol benzene/mol and x6 = 0.190 mol toluene/mol enters a distillation column. The distillate of the column leaves the process at n7 = 668.0 mol/h and contains y7h = 0.9000 mol benzene/mol and y7 = 0.1000 mol toluene/mol. The bottoms of the column contains X8b = 0.250 mol benzene/mol and xgt = 0.750 mol toluene/mol and is recycled back to the fresh feed. Hydrogen is fed into the process at ni = 1183 mol H,/h. This process is carried out at 760 mmHg. A n, mol/h mol H/mol YSH2 YSCH, mol CH_/mol Ysh mol b/mol Ys mol t/mol n̟ mol/h n, mol/h Condenser Улн, тol H/mol Усн,…
Use the chemical reaction below to answer the following questions HCI(aq) + NaOH(aq) → NaCl (aq) + H2O (I) AH298 = -58 kJ/mol (a) How much heat is produced when 200 mL of 0.3 M HCL (density = 1.00 g/mL) and 250 mL of 0.25 M NaOH (density = 1.00 g/mL) are mixed? (b) If both of the solutions at the same temperature and the heat capacity of the products are 5.39 J/g °C , how much will the temperature increase? (c) What assumptions are made when calculating your answers
Portland Cement is manufactured by the dry process conforming to the following specifications: Lime Saturation Ratio: - (CaO +1.5 Mg0 - 0.7 SO3)100 2.85 SiO₂ + 1.18Al2O3 + 0.65 Fe₂03 92 Iron Ratio = Al₂O3 = 2 Fe₂03 Magnesia, MgO should not exceed 1.5% and Sulfur as SO3 is 2.2% by wt Silica content of 24% by wt is acceptable The above cement is manufactured in a rotary kiln using limestone and clay as raw materials mixed in 75:25 proportion by weight. Analysis of Raw Materials Component Limestone,% Clay, % CaO 54.5 7.13 Fe₂O3 0.42 7.68 Al₂O3 0.83 17.15 SiO₂ 1.72 55.14 MgO 0.85 2.16 CO₂ 41.68 10.74 100 100 In the kiln, coal is added to supply heat of combustion. Coal contains 67.2%C, 4% H, 1.7% S, 2.2% 0, 2.6% H₂O and 22.3% ash. Its gross calorific value is 25.62 MJ/kg on a dry ash-free basis. Air supplied is 10% in excess at 27°C, 100 kPa and 75% RH. The stack gas contains 23.5% CO₂. The clinker is cooled and gypsum (essentially pure CaSO4) amounting to 3% its mass is added. The final…
A CHM student completing the calorimetry experiment mixes 20.0 mL of 1.10 M HCl (aq) with 20.0 mL of 1.05 M NaOH (aq), and observes the temperature increase of 6.611∘∘C. Assume that the density of each solution is 1.02 g/mL, and the specific heat for the resulting solution is 4.02 J/g∙℃. Calculate the change in enthalpy for this reaction (ΔHrxn) in kJ/mol H2O. Use the correct sign (+ or -) and significant figures.
9.12 A 50 wt% Ni-50 wt% Cu alloy is slowly cooled from 1400°C (2550 F) to 1200°C (2190 F). (a) At what temperature does the first solid phase form? (b) What is the composition of this solid phase? (c) At what temperature does the liquid solidify? (d) What is the composition of this last remaining liquid phase?
Calculate the amount of heat required to pass through each section of the graph. Here are the heat capacities and phase change enthalpies of water. ΔHfus or enthalpy of fusion or the first phase change from solid to liquid ΔHfus = 6.01kJ/mol ΔHvap or enthalpy of vaporization or the second phase change from liquid to gas ΔHvap = 40.7kJ/mol cliquid water or specific heat of water in the liquid phase cliquid water = 4.184J/g℃ cice or specific heat of water in the solid phase cice = 2.108J/g℃ cwater vapor or the specific heat of water in the gas phase cwater vapor= 1.996J/g℃
..
4. At 1084 °C solid copper melts to form a liquid. The phase change can be described as Cu(s) → Cu(t). The density of solid and liquid copper are 8.96 g/cm' and 7.75 g/cm' respectively. The enthalpies of combustion of the solid and liquid are -156.06 kJ/mol and -167.92 kJ/mol respectively. The product of combustion of both the solid and liquid is CuO(s). Calculate the standard enthalpy changes for the fusion process in kJ/mol. Calculate the change in internal energy when the sample is under a pressure of 500 kbar. Cu(s) → Cu(e) Solid copper liquid copper enthalples of combustion 8.96 g/cm3 7.75 g 1cm² said: -156.06 kJ/mol liquid-162.42 kJ/mol

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