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18. Assuming CO2 to be an ideal gas, calculate the work done by 10 g of CO2 in expanding isothermally and reversibly from a volume of 5 liters to 10 liters at 27°C. What are q, AE, and AH for the process?

18. Assuming CO2 to be an ideal gas, calculate the work done by 10 g of CO2 in expanding isothermally and reversibly from a volume of 5 liters to 10 liters at 27°C. What are q, AE, and AH for the process?

Introduction to Chemical Engineering Thermodynamics
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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18. Assuming CO2 to be an ideal gas, calculate the work done by 10 g of CO2 in expanding isothermally and reversibly from a volume of 5 liters to 10 liters at 27°C. What are q, AE, and AH for the process? 22. For a certain gas the van der Waals constants are a = 6.69 atm-liter²/mole² and b = 0.057 liter. What will be the maximum work performed in the expansion of 2 moles of the gas from 4 to 40 liters at 300°K? 25. Eight grams of O2 at 27°C and under a pressure of 10 atm are permitted to expand adiabatically and reversibly until the final pressure is 1 atm. Find the final temperature and the work done in the process. Assume that C, = ½ R for O2.
Transcribed Image Text:18. Assuming CO2 to be an ideal gas, calculate the work done by 10 g of CO2 in expanding isothermally and reversibly from a volume of 5 liters to 10 liters at 27°C. What are q, AE, and AH for the process? 22. For a certain gas the van der Waals constants are a = 6.69 atm-liter²/mole² and b = 0.057 liter. What will be the maximum work performed in the expansion of 2 moles of the gas from 4 to 40 liters at 300°K? 25. Eight grams of O2 at 27°C and under a pressure of 10 atm are permitted to expand adiabatically and reversibly until the final pressure is 1 atm. Find the final temperature and the work done in the process. Assume that C, = ½ R for O2.
35. Suppose that a gas obeys at low pressures the equation B PVm = RT + ( A + where A and B are constants independent of pressure and temperature, and Vm is the molar volume. Derive the expression for the change in enthalpy which will accompany the expansion of n moles of gas from a pressure P2 to a pressure P1 at temperature T. 39. For CO:(g) at 300°K and 1 atm pressure (дН/ӘР)т %—D —10.2 сal mole-1 atm-' and C, cient of the gas for the given temperat:ıre and pressure conditions. = 8.919 cal mole¬' degree¬1. Calculate the Joule-Thomson coeffi- 45. Compare the thermodynamic efficiencies to be expected: (a) When an engine is allowed to operate between temperatures of 1000°K and 300°K. (b) When an engine is allowed to operate between 1000°K and 600°K, and then the waste heat is passed on to another engine which operates between 600°K and 300°K.
Transcribed Image Text:35. Suppose that a gas obeys at low pressures the equation B PVm = RT + ( A + where A and B are constants independent of pressure and temperature, and Vm is the molar volume. Derive the expression for the change in enthalpy which will accompany the expansion of n moles of gas from a pressure P2 to a pressure P1 at temperature T. 39. For CO:(g) at 300°K and 1 atm pressure (дН/ӘР)т %—D —10.2 сal mole-1 atm-' and C, cient of the gas for the given temperat:ıre and pressure conditions. = 8.919 cal mole¬' degree¬1. Calculate the Joule-Thomson coeffi- 45. Compare the thermodynamic efficiencies to be expected: (a) When an engine is allowed to operate between temperatures of 1000°K and 300°K. (b) When an engine is allowed to operate between 1000°K and 600°K, and then the waste heat is passed on to another engine which operates between 600°K and 300°K.
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