one mole of an ideal gas is expanded isothermally against a constant pressure of 3 atm from 10 litre to 35 litre. calculate work, change in internal energy and heat
Answers
Answered by
3
Answer:
As the gas is expanded against constant pressure so,
Work done, W=−PΔV
V
2
= final volume =2.5 L
V
1
= initial volume =300 cm
3
=0.3 L
P is constant external pressure =1.9 atm
W=−P(V
2
−V
1
)
=−1.9×(2.5−0.3)
=−4.18 L.atm
In joules we know,
1 atm.L=101.325 J
Hence, −4.18 L.atm=−4.18×101.3=−423.5 J
Similar questions