A simultaneous dehydration reaction of liquid 2-methyl-2-butanol (A) produces 2-methyl-2- butene (B) and 2-methyl-1-butene (C) as shown in Figure 1 was carried out in a two continuous stirred tank reactor (CSTR) connected in series. The dehydration of A to B occur in second order whereas dehydration to C was in first order. CH3 k1 CH3 CH, C=CH-CH₂ 2-methyl-2-butene (B) CH₁₂ -CH2-CH3 CH₂ k₂ ОН CH₂-C-CH₂-CH₂ 2-methyl-2-butanol(A) 2-methyl-1-butene(C) Figure 1 Dehydration reaction of liquid 2-methyl-2-butanol a) Inlet stream consists of pure A with concentration of 40 mol dm³ and constant volumetric flowrate of 2 m³-min¹. The concentration of A at the exit stream of reactor one was reduced to 50%. The composition of product leaving reactor one consists of 60% B and 40% C. If the size of reactor one is 5 m³ and reactor two is double of reactor one, determine the composition of remaining A, product B and C in the exit stream of reactor two.

Problem 3 Dibutyl phthalate (diester) is produced in a CSTR operated isothermally at 112°C. The rate of formation of the di-ester from phthalic anhydride and butanol being very fast, the controlling step, in the presence of sulphuric acid catalyst, is the conversion of mono-ester to the diester. The liquid phase reaction is: СЫН.(СООCН:)CООН + CН,ОН A C6H4(COOC4H6)2 + H2O D B The rate of the reaction is given by the expression -TA = kC; gmol/L.h where CA is the concentration of the mono-ester in gmol/L. The value of the apparent rate constant is given by: k = 0.7628 x 10ol1.965- L/gmol.h where T is the reaction temperature in K. The initial concentration of the mono-ester is 2.84 gmol/L and the density of the reaction mixture is 0.984 kg/L. (Molar mass of diester = 278) 1. In an existing plant consisting of a CSTR of 1.1 m diameter and 1.6 m height, the volumetric feed rate is 10 L/min. (a) Find the conversion achieved in an ideal CSTR. (b) If the conversion achieved in practice 68.5%…

Now, let's use what we know about chemistry to infer how much acetic acid was in our sample. Let's look closely at the equation for the reaction we performed. HC2H3O2(aq) + NaHCO3(s) → NaC2H3O2(aq) + H2O(1) + CO2(g) Based on this balanced chemical reaction, we can see that for every one mole of CO2 that was produced one mole of acetic acid was consumed. Based on this, calculate the moles of acetic acid and grams of acetic acid that must have reacted in each sample. Sample Data for Vinegar Lab moles CO2 Produced Moles HC2H3O2 Consumed g HC2H302 Consumed by by Reaction by Reaction Reaction -2 g NaHCO3 0.0329 -4 g NaHCO3 0.0464 -6 g NaHCO3 0.0523 -8 g NaHCOз 0.0477 -10 g NaHCO3 0.0489

when acetone is heated in the gas phase, decomposition into ketene and methane takes place according to: (CH3)2CO > CH2-CO + CH4 the reaction is irreversible and first order. The rate constant is 1.047 s-1 vid 725 C. Calculate the turnover of acetone obtained in an isothermal and isobaric tube reactor under the following operating conditions. The reactor is made up of 20 parallel connected tubes, each with a length of 10 meters and an inner diameter of 10 cm. The working pressure is 4 atm and the temperature is 725 C. The acetone supply amounts to 120 mol/s.

When N2O5(g) is heated it dissociates into N2O3(g) and O2(g) according to the following reaction: N2O5(g)⇌N2O3(g)+O2(g)Kc=7.75N2O5(g)⇌N2O3(g)+O2(g)Kc=7.75 at a given temperature. The N2O3(g) dissociates to give N2O(g) and O2(g) according the following reaction: N2O3(g)⇌N2O(g)+O2(g)Kc=4.00N2O3(g)⇌N2O(g)+O2(g)Kc=4.00 at the same temperature. When 4.00 mol of N2O5(g) is heated in a 1.00-L reaction vessel to this temperature, the concentration of O2(g) at equilibrium is 4.50 mol/L. A. Find the concentration of N2O5 in the equilibrium system. B. Find the concentration of N2O in the equilibrium system C.Find the concentration of N2O3 in the equilibrium system.

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11.4 mole dichloromethane (CH2Cl2) enter a reactor with 20.6 mole hydrogen (H2) and 38.6 mole oxygen (O2).  The following reaction takes place: CH2Cl2 + H2 + 3/2 O2 → COCl2 + 2 H2O The extent of the reaction is 6.8. Calculate the mole of H2O that are produced.

Consider the pair of reactions in which ethylene is oxidized either to ethylene oxide (desired) or to carbon dioxide (undesired) in the furnace: C₂H4+0₂-C₂H4O C₂H₂ +30₂-2 CO₂ + 2H₂O The feed mixture and air are fed at a temperature To. All gaseous effluents are at temperature T emerging from the non-isothermal reactor. a) Calculate the number of degrees of freedom of the process. How would the answer differ if the reactor were adiabatic? b) Outline a manual calculation procedure to determine the compositions of all streams.

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Direct dehydrogenation of ethylbenzene to styrene is carried out in the vapor phase with steam over a catalyst consisting primarily of iron oxide. The reaction is endothermic, and can be accomplished either adiabatically or isothermally. Both methods are used in practice. The major reaction is the reversible, endothermic conversion of ethylbenzene to styrene and hydrogen: C6H3CH₂CH CoHsCHCH₂ + H₂ AH= 124.9 kJ/mol Competing thermal reactions degrade ethylbenzene to benzene C6H3CH₂CH3C6H6+ C₂H4 AH 101.8 kJ/mol Styrene also reacts catalytically to toluene: CH3CH₂CH3 + H2 CH3CH3 + CH4 AH=64.5 kJ/mol The reactions take place at 620°C. The costs are as shown in Table 1. The production rate of styrene is 200 mol/h. Chemical name Formula Cost (S/kmol) Ethylbenzene C6H5CH₂CH3 57.1 Styrene C.HSCHCH₂ 75.9 Benzene C6H6 32.8 Toluene C6H5CH3 25.8 Hydrogen H₂ 1.2 (as fuel) Methane CH4 4.0 (as fuel) Ethylene C₂H4 6.7 (as fuel) Correlation for the product selectivity and distribution are given as…