Question

A 1.0 mol of ideal gas, initially at 10 atm and 300 K is
allowed to expand isothermally to 1.0 atm, as follows:
(a) Reversible expansion to 5 atm followed by
(b) Irreversible expansion against 1.0 atm
Determine the net work done by the system and describe
the whole processes on p-V diagram.​

Answer 1

Answer:

Explanation:

Calculate the workdone individually

For W(reversible) it is -nRTln pi/pf or ln Vf/Vi

And for next half W[irreversible] it is -p[Vf-Vi]

And calculate volume through the formula PV=nRT and then p1/p2=V2/V1

Answer 2

the net work done by the system 3.724 KJ

given: A 1.0mol of ideal gas, initially at 10atm and 300 K is

allowed to expand isothermally to 1.0atm

to find:  the net work done by the system

solution:

Pi= 10atm

Pf= 1atm

since the gas is isothermal at 300k

for reversible reaction

w = -nRT㏑(Pi/Pf)

for irreversible

w = P[Vf-Vi]

using ideal gas equation

PV=nRT

n=1

so V= RT/P

Vf = 300R

Vi = 60R

Wrev = -1×8.314×300 ㏑(10/5)

= -1729.16 J

= -1.729 KJ

Wirrev =-1[300R-60R]

=-240 × 8.314

=1.995 KJ

net work  = Wrev + Wirrev

= -1.729 - 1.995

=-3.724 KJ

hence the net work done by the system 3.724 KJ

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