A reactor with an internal capacity of 160. L is charged with 75.0 atm of N2 gas and 145 atm of H2 gasat a reactor temperature of 200 °C. The two gases react to produce ammonia according to the followingequation.N2(g) + 3H2(g) → 2NH3(g)(a) Which is the limiting reactant, N2 or H2? (b) When the limiting reactant is completely reacted andthe reaction has 100% yield, what is the partial pressure of NH3 gas produced at the reactor temperatureof 200 °C? What is the partial pressure of NH; after the gas is cooled to 25°C?

Write the reaction as follows: N2g + 3H2g → 2NH3g 1 mole of N2 reacts with 3 moels of H2 and forms…

Answered: A reactor with an internal capacity 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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Consider the following dissolution of lead(II) fluoride (PbF>(s): O 5.9 kJ molr1 PbF>(s) - Pb2*(ag) + 2 F(ag) O 5.9 kJ mol1 Below is a table of thermodynamic quantities pertaining to this reaction: Submit Request Answer Substance AHP (kJ mol1) S° (J K-1 mol1) Part B PBF2(s) -664.0 110.5 Determine the standard entropy of reaction (A,S°) for the dissolution of lead(II) fluoride. Pb2*(aq) 0.9 18.5 O 119.6 J K1 mol1 F(ag) -335.4 -13.8 O -105.8 J K1 mor1 O 119.6 J K1 mor1 O 105.8 J K-1 mol1
The conversion of ethane to ethylene is a gas phase dehydrogenation reaction that takes place at P = 1 bar and T = 25 °C. The chemical reaction is given below: 2426 2 H HC HC +Determine the standard Gibbs Energy of the reaction (Δ?? 0) and the equilibrium constant (KT).
Absolute (100%) ethanol is produced from 95% ethanol and 5% water using the Keyes distillation process. Another component, benzene, is added to lower the instability of the alcohol. With these conditions, the product from the top of the distiller is a constant-boiling mixture of 18.5% ethanol, 7.4% H₂O, and 74.1% benzene, as shown here: 95% ethanol 5% water Benzene Distillation tower P(absolute ethanol) = 0.785 g/cm³ P(benzene) = 0.872 g/cm³ 74.1% benzene 18.5% ethanol 7.4% water 100% ethanol Calculate the volume of benzene that should be fed to the still to produce 250 L of absolute ethanol, using this data:
1. An impure sample of compound A is contaminated with two impurities B and C. The sample is to be purified by recrystallization using ethanol as the solvent. The solubility properties of the three components are summarized below. Solubility in Solubility in ethanol Solubility in 50 mL Solubility in 50 mL ethanol at -78 °C at - 0°C ethanol at -78 °C ethanol at - 0°C (g) (g) Compound A 0.12 g/mL 0.02 g/mL Impurity B 0.58 g/mL 0.04 g/mL Impurity C 0.005 g/mL 0.0003 g/mL The impure (7.5 g) sample contains 5.0 g of compound A, 1.5 g of B and 1.0 g of C and is recrystallized using 50 mL of ethanol. The sample is boiled with 50 mL of ethanol, filtered by gravity and then cooled in ice and filtered by suction. a) How much compound A should be obtained as the final product? Will the sample be contaminated with any of the impurities? Explain (using calculations to support your answer-fill in the missing masses in the table above). Hint: For this question you should calculate the mass of each…
Consider the following reaction in a sealed vessel kept at constant temperature: A(g) ⇌ 2B(g) If the reaction is started with 2.0 mol of A and no B, the amount of B at equilibrium is 3.0 mol. How many moles of A should one start with to obtain 6.0 mol of B at equilibrium under the same conditions (same vessel, same temperature, no gas B present initially)? A. 5.6 mol B. 5.0 mol C. 4.0 mol D. 6.0 mol E. 6.5 mol
Consider the dissociation of methane to graphite (C) and hydrogen gas. For the methane at 298K, the data available are: k] -74.85- mol = -80.67- mol · K A,GEgraphite = A,G Calculate the equilibrium constant (K) of the dissociation of methane a. at 298 K with the appropriate units. b Assuming that A,H is independent of temperature, calculate the equilibrium constant (K) of methane dissociation at 1000 K. Calculate the ratio between the amounts of methane and hydrogen C. gases at 298 K and 0.2 barg.
Oxygen can be converted into ozone by the action of lightning or electric sparks: 302(g) 2 203(g) For this reaction, AH = and K = 2.68 × 10¬29 at 25 °C. +68 kcal/mol (+285 kJ/mol) %3D (a) Is the reaction exothermic or endothermic? (b) Are the reactants or the products favored at equilibrium? (c) Explain the effect on the equilibrium of (1) increasing pressure by decreasing volume. (2) increasing the concentration of O2(g). (3) increasing the concentration of O3(g). (4) adding a catalyst. (5) increasing the temperature.
The decomposition of N,0, can be described by the equation 2 N,0,(soln) → 4NO, (soln) + O,(g) Consider the data in the table for the reaction at 45 °C in carbon tetrachloride solution. 1 (s) [N,O3] (M) 2.576 215 2.250 456 1.934 755 1.602 Given the data, calculate the average rate of reaction for each successive time interval. What is the average rate of reaction for the time interval from 0 s to 215 s? average rate of reaction: M/s What is the average rate of reaction for the time interval from 215 s to 456 s? average rate of reaction: M/s What is the average rate of reaction for the time interval from 456 s to 755 s? average rate of reaction: M/s
You are in a research & development team responsible for generating preliminary data for the following gas-phase reaction: CO₂(g)+ 4H₂ (g) → 2 H₂O (g) + CH.(g) The reaction occurs over a catalyst at a reactor pressure of 1 atm and 500 C and goes essentially to completion. Use the following heat capacities data for your calculation: CO₂ (g): H₂ (g): H₂O (g): CH₁ (g): Cp=0.0451 kJ/mol C Cp = 0.0291 kJ/mol C Cp = 0.0358 kJ/mol C Cp=0.0487 kJ/mol C a) Calculate the standard heat of reaction (kJ/mol). (-165.01 kJ/mol) b) If the gases enter and leave the reactor at 1 atm and 500 C, what is the heat of reaction at 500 C (i.e. Ê, at 500 C) in kJ/mol. Assume the reactants are fed in stoichiometric amounts. (-184.63 kJ/mol)
1. Cyclohexane can be produced from the hydrogenation of benzene according to the reaction C6H6 (g) + 3 H2 (g) --> C6H12 (g) Ka = 1.371 at 550 K The reactor temperature is 550K and hydrogen to benzene feed mole ratio is 4.5:1. Estimate the gas composition under equilibrium conditions if the reactor pressure is 30 bar. The following fugacity coefficients are obtained for the species involved: Fugacity coefficient (550K, 30 bar) Cyclohexane 0.907 Benzene 0.919 Hydrogen 1.003
The equilibrium constant for the reaction of nitrogen and hydrogen to give ammonia is 0.118 at 745 K. The balanced equilibrium equation is as follows: N2(g) + 3H₂(g) = 2NH3(g) What is Kp for this reaction at the same temperature? (R: 0.082 L atm/mol.K)
A student determines the value of the equilibrium constant to be 1.98×10-5 for the following reaction.CO2(g) + H2(g)CO(g) + H2O(g)Based on this value of Keq:G° for this reaction is expected to be (greater, less) fill in the blank 1 than zero.Calculate the free energy change for the reaction of 1.74 moles of CO2(g) at standard conditions at 298K. G°rxn = kJ

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