One mole of air, initially at 148°C and 8 bar, undergoes the following mechanically reversible changes. It expands isothermally to a pressure such that when it is cooled at constant volume to 50°C, its final pressure is 3 bar. Assuming air is an ideal gas for which Cp= (7/2)R and Cy= (5/2)R, calculate the work done (W), the heat transfer required (Q), the change in internal energy (AU), and the change in enthalpy (AH). The values of Rare given in the following table: Values of the Universal Gas Constant R = 8.314 J-mol-K- = 8.314 m³-Pa-mol-.K- = 83.14 cm-bar-mol-K = 8314 cm³-kPa-mol-K! = 82.06 cm-(atm)-mol K = 62, 356 cm³-(torr)-mol-K- = 1.987 (cal)-mol-K = 1.986 (Btu)(lb mole) (R) = 0.7302 (ft) (atm) (lb mol)'(R)-1 = 10.73 (ft) (psia) (Ib mol)(R)- = 1545 (ft) (lb) (lb mol)(R)¯ The work done is - 3433.09 8 J-mol. The heat transfer required is 2851.702 * J-mol". The change in internal energy is - 2036.93 J-mol. The change in enthalpy is - 2851.702 J-mol1.
One mole of air, initially at 148°C and 8 bar, undergoes the following mechanically reversible changes. It expands isothermally to a pressure such that when it is cooled at constant volume to 50°C, its final pressure is 3 bar. Assuming air is an ideal gas for which Cp= (7/2)R and Cy= (5/2)R, calculate the work done (W), the heat transfer required (Q), the change in internal energy (AU), and the change in enthalpy (AH). The values of Rare given in the following table: Values of the Universal Gas Constant R = 8.314 J-mol-K- = 8.314 m³-Pa-mol-.K- = 83.14 cm-bar-mol-K = 8314 cm³-kPa-mol-K! = 82.06 cm-(atm)-mol K = 62, 356 cm³-(torr)-mol-K- = 1.987 (cal)-mol-K = 1.986 (Btu)(lb mole) (R) = 0.7302 (ft) (atm) (lb mol)'(R)-1 = 10.73 (ft) (psia) (Ib mol)(R)- = 1545 (ft) (lb) (lb mol)(R)¯ The work done is - 3433.09 8 J-mol. The heat transfer required is 2851.702 * J-mol". The change in internal energy is - 2036.93 J-mol. The change in enthalpy is - 2851.702 J-mol1.
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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Transcribed Image Text:One mole of air, initially at 148°C and 8 bar, undergoes the following mechanically reversible changes. It expands isothermally to a
pressure such that when it is cooled at constant volume to 50°C, its final pressure is 3 bar. Assuming air is an ideal gas for which Cp=
(7/2)R and Cy= (5/2)R, calculate the work done (W), the heat transfer required (Q), the change in internal energy (AU), and the change
in enthalpy (AH). The values of R are given in the following table:
Values of the Universal Gas Constant
= 8.314 J-mol-1-K-1 = 8.314 m³.Pa•mol-1-K-1
= 83.14 cm³-bar-mol-1-K-1
82.06 cm³ -(atm)-molK-' = 62, 356 cm³ (torr)-mol1-K-
1.987 (cal)-mol.K1
0.7302 (ft)° (atm) (lb mol)-' (R)-1 = 10.73 (ft)° (psia) (lb mol)- (R)-1
1545 (ft) (lbf) (lb mol)(R)
R
8314 cm³ -kPa-mol¬1-K-1
= 1.986 (Btu)(lb mole) (R)-1
The work done is - 3433.09
O J-mol-1.
The heat transfer required is |2851.702
O J-mol1.
The change in internal energy is - 2036.93
J.mol"1.
The change in enthalpy is -
J.mol"1.
2851.702
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