Hydrogen is a gas used as a fuel in different types of fuel cells, such as phosphoric acid,solid oxide and proton-exchange membrane fuel cells. This fuel can be obtained fromnatural gas through the following reactions:Steam-Methane Reforming:CHĄ(g) + H20(g) → co(g) + 3H2(g)AAÇ = 206.16 kJ/molWater-Gas Shift Reaction:CO2(g) + H2(g) → CO(g) + H20(g)ARÇ = 41.15 kJ/mol(i)Determine the enthalpy of the following reaction by applying Hess's Law:2CH,(g)+3H,0(g) → CO(g) + CO2(g)+ 7H¿(g)(ii)Verify the value obtained in Q1.(i) via the standard heat of formation.

Hydrogen as a fuel is produced from the methane in fuel cell. following reaction takes place in fuel…

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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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An A-B alloy of 70% B composition cools slowly from 1000°C to 200°C. Choose the correct option(s): a) A mixture of 70% B composition begins to form B crystals at 600°C b) A mixture of 20% B composition begins to form alpha crystals at approx. 820°C c) Alpha is a solid solution of A dissolved in B d) In the Liquido region there are 2 degrees of freedom e) A mixture at 40%B at 600°C has a composition solution approximately 47% B f) A mixture of composition 80%B has a solution of composition 86% B
59. Encode the solution.
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.
The first synthesis of chlorine gas was achieved in 1774 by oxidizing NaCl(aq) and H2SO4(aq) with solid manganese (IV) oxide, MnO2, as follows: NaCl(aq) + H2SO4(aq) + MnO2(s) à Na2SO4 (aq) + MnCl2 (aq) + H2O + Cl2(g) In a pilot scale verification, 0.5 kg of MnO2 were reacted with 85% by mass H2SO4(aq), containing 0.5 kg solute, and 80% by mass NaCl(aq), containing 0.5 kg solute. The products were sent to a separator where gaseous products are separated from the solution. During the process of separation, 12% of water produced vaporized. Assuming 100% completion, calculate the % compositions of the solution and the gaseous streams.
The fuel in the form of biogas (65%-mol CH4 and 35%-mol CO2) is burned in a furnace. In order for combustion to take place stoichiometrically, calculate the air to fuel ratio (vol/vol) from this problem!
Determine the heat of the reaction for the process: FeO(s) + Fe203(s) -> Fe3O4(s) given the following information: + O20 AHxn° = - 544.0 KJoules 2Fe(s) 4Fe(s) Fe;O4(s) ) + 302g) 3Fe(s) 2FEO(s) 2FE203(s) AHrxn° = - 1,648.4 KJoules + 202(g) AH° = 1.118.4 KJoules
A chemical engineer is studying the following reaction: BF 3(aq)+NH3(aq) → BF ,NH3(aq) At the temperature the engineer picks, the equilibrium constant K for this reaction is 1.3. The engineer charges ("fills") three reaction vessels with boron trifluoride and ammonia, and lets the reaction begin. He then measures the composition of the mixture inside each vessel from time to time. His first set of measurements are shown in the table below. Predict the changes in the compositions the engineer should expect next time he measures the compositions. reaction expected change in concentration compound concentration vessel BE3 I decrease (no change) 0.48 M f increase NH3 I decrease (no change) 0.55 M f increase A BF,NH3 f increase I decrease (no change) 1.01 M 0.41 M f increase I decrease (no change) BF, NH3 I decrease (no change) 0.48 M f increase В BF,NH3 f increase I decrease (no change) 1.08 M BF3 I decrease (no change) 1.07 M ↑ increase NH3 I decrease (no change) 1.14 M f increase C…
3.19 Crude calcium carbide, CaC2, is made in an electric furnace by the following reaction. Cao + 3C –→ CaC, + CO The product contains 85% CaC, and 15% unreacted CaO. (a) How much CaO is to be added to the furnace charge for each 1000 kg CaC2? (b) How much of CaO is to be added to the furnace charge for each 1000 kg of crude product?
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
The gas acetylene is produced according to the following reaction by treating calcium carbide with water: CaC₂ + H₂O → C₂H₂ + Ca(OH)2 Calculate the number of hours of service that can be derived from 2 kg of carbide in an acetylene lamp burning 0.06 m³ of gas per hour at a temperature of 24ºC and a pressure of 743 torr.
1.Calculate the heat of formation of PCI5 (cr), given the heats of the following reactions at 25C: 2P (cr) + 3Cl2(g) = 2PCI3 (1) PCI3 (1)+ Cl2 (g) = PCI5 (cr) H = -635.13 kJ /mole H = -137.28 kJ / mole

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