3) A zero-order homogeneous gas reaction A rR proceeds in a constant-volumebomb, 20% inerts, and the pressure rises from 1 to 1.3 atm in 2 minutes. If the samereaction takes place in a constant-pressure batch reactor, what is the fractionalvolume change in 4 minutes if the feed is at 3 atm and consists of 40% inerts.

A zero order reaction is carried out in constant volume and constant pressure reactor.

Answered: A zero-order homogeneous gas reaction A…

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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Please show every step you used to solve each problem. A vapor mixture of 100 mol/s comprising 55 mol% benzene and 45 mol % toluene is sent to a partial condenser operating at 760 mm Hg. 75 mol% of the toluene in the feed is recovered in the liquid product. Determine all unknown flow rates, compositions, and required heat removal. and do a degree a. Draw a process flow diagram of freedom analysis b. Write out equations used to solve and to calculate all specifications used in Excel Solver unknown flow rates, compositions, C. F Specify the temperature and pressure of the feed as T₁ = 102°C and P₁ = 760 mm Hg. Choose the lowest enthalpy stream (liquid product stream) for a reference condition. Calculate the required heat removal analytically by hand (No Excel Solver). d. Create Enthalpy Table
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Product B is produced in a batch reactor according to the elemental reversible reaction (A⇋B) in liquid phase. The reactor volume is 10 L and the reaction temperature is 60°C. The initial concentration of reagent A is 3 lbmol/L, the rate constant for the forward reaction is k1=6.0 h-1, and the rate constant for the reverse reaction is k2=0.53h-1. Determine: (a) Plot the concentration of each species as a function of reaction time(b) Plot the conversion as a function of reaction time
Q2- The synthesis of ammonia proceeds according to the following reaction N₂ + 3 H₂ -----> 2 NH3 In a given plant, 4202 lb of nitrogen and 1046 lb of hydrogen are fed to the synthesis reactor per hour. Production of pure ammonia from this reactor is 3060 lb per hour. a. What is the limiting reactant. b. What is the percent excess reactant. c. What is the percent conversion obtained (based on the limiting reactant).
Given the following reaction: A (s) + 2B (g) + heat 1. 2C (g) + 2D (g) Considering Le Châtelier's Principle, type in the boxes either no shift or shift to the right or shift to the left for each of the following cases: a) Using a catalyst b) [D] is decreased c) Volume is increased d) Temperature is decreased e) [C] is increased f) [A] is decreased
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A reactor is used for oxidation of a chemical compound. The reaction rate constant k is 0.8 h HRT is 4 h. The oxidation efficiency is 96%. Determine the flow regime in the reactor.
The formation of NO from Na and O is to be carried out in a small batch reactor. As a first approximation, we shall consider that the reaction time is more rapid than the time of cylinder compression, consequently, the reaction takes place isothermally in car eylinder at 2700 K, in a constant volume reactor (cylinder) and under a pressure of 20 atm, the initial concentration of N2 is 0.0696 mol/liter. By a specifying constant volume, we are assuming that reaction take place rapidly with respect to the movement of the piston in the cylinder. Consider that the feed consists of 77% N2, 15% Oz and 8% other gases, which may be considered inert. At this temperature the equilibrium constant (Ke-0.01). The reaction is reversible: Na + 0z + 2NO With a rate equation: Cho -TN, = k ( CN, Co, Ke Calculate: a) The equilibrium conversion of N2. b) The time required to achieve 80% of the equilibrium conversion. The formation reaction rate- constant k at this temperature is 1.11 liter mol.h' Hint: dx…

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