Evaluate the equilibriumconstant at 2000 K forCH+ HO 3H,+COAt 2000 K, log1o K=7.469 forC+CO, and log1oK=-3.408 forC+2H, CH,510 9.1737^10 2.173)710 9.1/39,17305 10 2173

Given that For the reaction C +12O2 ⇔CO log10K = 7.469C+2H2⇔CH4 log10K =-3.408

Answered: Evaluate the equilibrium constant at…

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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Explain why Raoult's Law has very limited applicability in its ability to accurately predict vapor-liquid equilibrium behavior. Be very specific in your answer.
Consider the following equilibrium system: N2 (g) + 3H2 (g) Ź 2NH3 (g) + 92.94 kJ For each, state what happens to the number of moles of nitrogen gas, N2, and why that occurs. (the shift) a. increasing the temperature f. removing some ammonia b. decreasing the temperature g. adding some ammonia c. decreasing the pressure h. removing some nitrogen с. 6.
Q3. The following information on the pressure-temperature diagram of nitrogen: P (atm) T(K) 0.123 33.3978 1.0 Triple point Critical point Normal boiling point Density of N₂(s): 1.03g/cm-³ N₂(1): 0.808g/cm-³ 63.15 126.19 77.35 Using this information, sketch a phase-equilibrium diagram of nitrogen and mark each point. Then, describe why the slope of each phase/phase equilibrium is positive or negative.
i need some help wuth this question.please help.
Book: Introduction to Chemical engineering Thermodynamics 8th edition, McGraw Hill, 2018
Consider the following reaction: 4 NH3(g) + 5 O2(g) = 6 H20(g) + 4 NO(g) Calculate AG at 547 K for a mixture of 2.3 bar NH3(g), 3.0 bar O2(g), 4.9 bar H20(g), and 3.6 bar NO(g). State whether or not the reaction is spontaneous at these conditions. **AG° values can be found in textbook appendix** O -929 kJ/mol ; spontaneous -929 kJ/mol ; nonspontaneous O 929 kJ/mol ; spontaneous O 929 kJ/mol ; nonspontaneous
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The standard Gibbs free energy of formation of NH3 is -16.5 kJ mol-¹ at 298 K. What is the reaction Gibbs free energy when the partial pressures of the N2, H2, and NH3 (treated as perfect gases) are 3.0 bar, 1.0 bar. and 4.0 bar, respectively? What is the spontaneous direction of the reaction in this case?
Help with the following question. Please show all steps and double check your answer.
This problem is (12.24) from a book "Thermodynamics and Statistical Mechanics An Integrated Approach by M. Scott Shell"

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Evaluate the equilibrium constant at 2000 K for CH,+H2O 3H2+CO