2 -a - Calculate the work done for 10 moles ofCH4 during an expansion from an initial volumeof 5.0 L to a final volume of 10.0 L. Duringexpansion, the pressure of CH4 varies from aninitial value of 50 atm to a final pressure of 25atm. When the pressure reaches 25 atm, theexpansion stops due to the fact that the gasenters into mechanical equilibrium with theexternal environment, whose pressure is alsomaintained at 25 atm. The process involveshigh pressures, CH4 cannot be considered asan ideal gas.Develop all calculations in detail.b - Is it possible, through an isothermalcompression, to liquefy CH4 from its initialstate of volume = 5.0 L and pressure = 50atm)? Justify your answer.Develop all calculations in detail. An answerwithout justification wil not be considered.Parameters of the van der Waals equationfor CH4, where P is pressure and V thevolume:nRTn'ap=V – nba = 2.26 atm*L^2*mol^-2b = 0.043 L*mol^-1Critical CH4 temperature: – 82.5 °C

SOLUTION for a As the expansion had proceeded to completion and it is not infinitesimally slow…

Answered: Develop all calculations in detail. An…

Develop all calculations in detail. An answer without justification will not be considered. Parameters of the van der Waals equation for CH4. where P is pressure and V the

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Question

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2 -
a - Calculate the work done for 10 moles of
CH4 during an expansion from an initial volume
of 5.0 L to a final volume of 10.0 L. During
expansion, the pressure of CH4 varies from an
initial value of 50 atm to a final pressure of 25
atm. When the pressure reaches 25 atm, the
expansion stops due to the fact that the gas
enters into mechanical equilibrium with the
external environment, whose pressure is also
maintained at 25 atm. The process involves
high pressures, CH4 cannot be considered as
an ideal gas.
Develop all calculations in detail.
b - Is it possible, through an isothermal
compression, to liquefy CH4 from its initial
state of volume = 5.0 L and pressure = 50
atm)? Justify your answer.
Develop all calculations in detail. An answer
without justification wil not be considered.
Parameters of the van der Waals equation
for CH4, where P is pressure and V the
volume:
nRT
n'a
p=
V – nb
a = 2.26 atm*L^2*mol^-2
b = 0.043 L*mol^-1
Critical CH4 temperature: – 82.5 °C

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