2. Ethanol is produced by the hydration of ethylene according to the first reaction below.However, some of the products are converted to diethyl ether according to the secondreaction.C2H4 + H20 – C,H;0H2C2H;OH - (C2H5)20 + H20The feed to the reactor contains ethylene, steam, and N2. An effluent analysis is given inthe following table:C2H439.12H2OCH;OH2.95(C2H3)20Component%molWith a basis of 100 kmol of effluent, determine the following:N245.080.2712.58b. (.) Determine the fractional conversion of ethylene.

Given Details The molar composition of the reactor effluent gas: Mole% of C2H4 = 39.12 Mole% of…

Answered: Ethanol is produced by the hydration 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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2. Combustion of fuels with air at high temperatures can produce nitrogen/oxygen compounds (NOx) as unwanted by products. Because these compounds are pollutants, they must be removed, and one process for doing so is called selective catalytic reduction (SCR). A researcher claims to have developed a new SCR catalyst that uses ammonia (NH3) as a reactant to convert NO into nitrogen and water via the reaction: 6NO(g) + 4NH3(g) ---> 5N2(g) + 6H₂O(g) We are working on the design for a process using this reaction in which 120 mol/hr of an equimolar mixture of NO and NH3 (i.e., 60 mol/hr NO and 60 mol/hr NH3) at 450°C is fed to the reactor. We may assume that the reaction goes to completion in the limiting reactant. The reactor is jacketed to maintain the temperature at 450°C, and we may assume that the pressure is held constant at 1 Atm. Use the following constant heat capacities for the (a) (b) | (c) [ Species NO (g) NH3(g) N₂ (g) H₂O (g) gases: C₂ (J/mol K) 30.5 37.0 29.1 34.2 Determine…
As reported in US Patent 4203923, cyclohexanone is an important chemical raw material in the production of nylon intermediates. The separation and purification section for cyclohexanone production usually done through a series of distillation units. Liquid mixture of cyclohexanone (1) and phenol (2) was reported to exist in equilibrium with its vapor at 144 °C (417.15K). The system conforms closely to Modified Raoult’s Law. The mixture forms azeotrope at composition of 0.695. (Refer Table) (a) Provide a sketch that clearly shows that the system exhibits azeotrope(α12)x1=0 = P1sat eA / P2sat and (α12)x1=1 = P1sat / P2sat eA (b) State Paz and sketch a P-xy diagram of the system
(a) Consider the following chemical reaction: 3FE203(s) + CO(g) → 2Fe304(s) + CO2(g) AH° = ? Use the following thermochemical data to determine the enthalpy change of this reaction. (6) 2FE2O3 (s) AH° = -1652 kJ 4Fe(s) + 302(g) C(s,graphite) + ½O2(g) → CO(g) 3Fe(s) + 202 (g) → CO2(g) AH° = -110.5 kJ Fe304(s) C(s,graphite) + O2(g) AH° = -1117 kJ AH° = +395.5 kJ (b) What is the standard enthalpy of formation of carbon dioxide? (2)
Methanol (CH3OH) and its derivative products are used as base materials in acrylic plastic, synthetic fabrics, adhesives, paints and as chemical agent in pharmaceuticals and agrichemicals. In petrochemical industry, one promising pathway to produce methanol is from conversion of syngas to methanol via hydrogenation of carbon dioxide and carbon monoxide. The reaction of this process is given as follows, CO + 2H2 → CH3OH (1) CO2 + H2 → CO + H20 (2) Suppose 1000 kmol/hr of syngas with molar composition of 22% CO2, 6.7% CO, 65% H2, 4.1% H20, 1.1% CH4 and 1.1% N2 is used as fresh feed. (a) Draw and label a complete process flow diagram of this process. (b) Calculate the amount of unreacted CO2 if given single pass conversion of CO2 is 14.2%. (c) Calculate the extent of reaction for the side reaction (2) and the amount of water produced. (d) If the selectivity of methanol to water is 92.1%, calculate the amount of methanol produced. (e) Determine mole fraction of CH3OH, CO2, CO, H2, H2O, CH4…
13.7 mole Boron Trichloride (BCl3) enter a reactor with 52.4 mole water for the following reaction: BCl3 + 3 H2O → H3BO3 + 3 HCl 18.2 mole HCl are formed. Calculate the fractional conversion of the limiting reactant.Note: fractional conversions go from 0 to 1
Please help with the material balances!!!!! Please!!
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%…
Basic Principles of Chemical Engineering Question Please solve step by step
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,…
#3 The first step in the reaction sequence for the production of nitric acid via the oxidation of ammonia is: 4NH3 + 502 2 4NO + 6H2O 75% conversion is achieved with an equimolar mixture of ammonia and oxygen fed at the rate of 100 mol/h. Determine the outlet compositions. (Hint: determine the limiting reactant).
Nitromethane, CH3NO2 , can be used as a fuel. When the liquid is burned, the (unbalanced) reaction is mainlyCH3NO2(l) + O2(g) → CO2(g) + N2(g) + H2O(g)a. The standard enthalpy change of reaction (ΔH°van ) for the balanced reaction (with lowest whole-number coefficients) is −1288.5 kJ. Calculate ΔHf0 for nitromethane.b. A 15.0-L flask containing a sample of nitromethane is filled with O2 and the flask is heated to 100.°C. At this temperature, and after the reaction is complete, the total pressure of all the gases inside the flask is 950. torr. If the mole fraction of nitrogen (χnitrogen) is 0.134 after the reaction is complete, what mass of nitrogen was produced?
Example 3: A vessel content, one mole of carbon dioxide is heated. The carbon dioxide is dissociated 1 as: CO₂ → CO + 0₂. 2 If the equilibrium constant is given as: Kp = 30 ln(T) – 240. After equilibrium occurs, the carbon monoxide mole fraction is 0.098 find the reached temperature of the mixture.

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