Question

Two moles of an ideal gas initially at 27°c
and one atmospheric pressure are
compressed isothermally and reversibly
till the final pressure of the gas is 10 atm.
Calculate q, W and ∆u for the process.​

Answer 1

Explanation:

Given,

T=(27+273)K=300K

∆T=0 ( As temperature is constant)

P1=1atm

P2=10atm

n=2 moles

As per question,

Work=2.303×2×8.314×300×log(10/1)

= 11488 J

Now,

∆U= 2×c×0= 0

Now, from 1st law of thermodynamics

∆U=q+W

0=q+W

q= -W

q= -11488 J

Formulas used,

W=2.303 nRT log(P2/P1)

∆U=q+W

∆U= nC∆T