Press Esc to exit full screen5.) The standard entropy change for the raction shownbelow at 298K is -266 J/mol·K. Calculate the standardentropy value of C,H4e) using the information shownbelow.Substance Entropy (S)205 J/mol-K214 J/mol K70 J/mol KCH4g)+ 30, 2H,02H,O@ + 2C022)

Given: Entropy Change for a Reaction = -266 J/mol K Entropy of O2 = SO2 = 205 J/mol K Entropy of…

Answered: 5.) The standard entropy change for the…

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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The saturation pressure for vapor–liquid equilibria for a given species is fitted tothe Antoine equation, ln (Pvap/Pref) = c1 - c2/(T + c3), where c1, c2, and c3 arematerial-specific constants. Assume the vapor obeys the equation of state P+NkBT/(V - Nb), where b is another constant that modifies the ideal gas expressionto account for molecular volume.(a) Write an expression for the enthalpy of vaporization as a function oftemperature.
enthalpy given a non-ideal gas equation of state Consider a gas that demonstrates the following equation of state: P(V - b) = RT Determine if enthalpy is only a function of T (like if a gas is ideal) or if it is a function of both T and P. solution guide: 1. Obtain the exact differential of H with respect to T and P. 2. Derive the exact differential to an equation which has Cp and 3. Obtain (3) P from the equation of state above. ат av and state your final answer. 4. Plug (37) p.
1. The Helmholtz function of a certain gas is given by (V – F (T,V) = –nRT |1+ ln v – nb)T? an? пф V where n is the number of moles of gas, T is the temperatures of the gas, V is the volume of the gas, and a, b, and o are constants. (a) Derive the equation of state, the entropy, and the internal energy of the gas. (b) Suppose that 100 moles of the gas expands from 2 m3 to 5 m³ at 280 K and that the constants have the values a = 0.364 J m3 mol-2, b = 4.27 × 10-5 m³ mol-1, and $ = 1.09 × 10-5 m³ K³/2 mol-1. Calculate: (i) AU. (ii) the maximum energy that can be made available for work due to the process.
1. Calculate AU, AH, q, and w for the reversible isothermal expansion of 62.4 g of Ar from a volume of 2.50 L to 15.5 L at 150.0 K. a. Treat Ar as an ideal gas. b. Treat Ar as a gas with the equation of state given below where a represents the van der Waals attraction constant. (We are ignoring the constant b in this problem.) а (P+ -)V = RT V? m т c. Explain any difference between your answers to parts a and b.
Whenever a substance is heated, its enthalpy increases, as suggested by the relation, ∆?=Cp∆?. However, the molar heat capacity itself is a function of temperature, and for N2 this function can be modeled as ?p(?)=? + ?? + c / T2 where a= 28.58 J/mol·K, b= 0.00377 J/mol·K2, and c= –5.0 x 104J·K/mol. (a) What does this formula for heat capacity predict for the value of ?p(?)at 300K? (b) Now, compute the enthalpy change associated with heating 0.62 moles of N2 from 300 to 600 K using the formula for ?p (?), and report the answer in J. (c) What is the difference between this value and one computed using the constant value for Cp at 300 K from part (a)? Report the absolute value of the difference in J.
13 An ideal solution of 5.25 moles of benzene and 3.0 moles of toluene is placed in a piston and cylinder assembly. At 298 K, the vapor pressure of pure substances are P°(benzene) = 96.4 torr & P°(toluene) = 28.9 torr. The vapor pressure of the solution is; 69.81 torr O 71.83 torr 53.47 torr O 66.61 torr 67.50 torr
For a van der Waals gas: (∂Um∂V)=aV2m In this problem, you will compare the change in energy with temperature and volume for N2, treating it as a van der Waals gas. 1) Calculate ΔU per mole of N2(g) at 1 bar pressure and 298 K if the volume is increased by 7.00 % at constant T. Approximate the molar volume with the ideal gas value. a(N2)=1.370dm6⋅bar⋅mol−2 .Express your answer with the appropriate units. 2) Calculate ΔU per mole of N2(g) at 1 bar pressure and 298 K if the temperature is increased by 7.00 % at constant V. CP,m for N2(g) at 298 K is 29.13 J⋅K−1⋅mol−1 .Express your answer with the appropriate units.

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5.) The standard entropy change for the raction shown below at 298K is -266 J/mol·K. Calculate the standard entropy value of C,H4) using the information shown below. Substance Entropy (S) Oz2) CO 268) 205 J/mol K 214 J/mol·K H,O 70 J/mol K C,H4) + 30, 2H,0@ + 2CO2«)