wiz-icon
MyQuestionIcon
MyQuestionIcon
1
You visited us 1 times! Enjoying our articles? Unlock Full Access!
Question

Calculate the work done by system in an irreversible (single step) adiabatic expansion of 1 mole of a polyatomic gas (γ=1.33) from 300K and pressure 10 atm to 1 atm.

Open in App
Solution

Given:-
Initial temperature (T1)=300K
Final temperature (T2)=T(say)=?
Initial pressure (P1)=10atm
Final pressure (P2)=1atm
γ=1.33=43
For an adiabatic process,
TγPγ1=constant
(T1T2)γ=(P1P2)γ1
(300T)=(101)11γ
300T=(10)14
T=3001.77=168.72K=T2
ΔT=(168.72300)=131.28K
Therefore, for an addiabatic expansion,
W=nCVΔT
W=1×Rγ1×(131.28)
W=3R×(131.28)=393.84R
Hence work done by the system will be 393.84R.

flag
Suggest Corrections
thumbs-up
0
Join BYJU'S Learning Program
similar_icon
Related Videos
thumbnail
lock
Introduction
CHEMISTRY
Watch in App
Join BYJU'S Learning Program
CrossIcon