1 mole of an ideal gas undergoes reversible isothermal expansion

thermodynamics
cbse

#1

1 mole of an ideal gas undergoes reversible isothermal expansion from an initial volume of ${ V }{ 1 }$ to a final volume of 10
${ V }
{ 1 }$ and does 10 kJ of work. The initial pressure was 1 x ${{10}^{7}}$ Pa.
(i) Calculate ${ V }_{ 2 }$
(ii) If there were 2 moles of gas, what must its temperature have been?


#2

(i) We know that W = — 2.303 nRT logV2/V1
10 x ${{10}^{3}}$ J = 2.303 x 1 x 8.314 x T x log 10V1/V1
T = 522.3K
For initial conditions, p1V1 = n1RT

If there were 2 moles of the gas, applying p1 V1 = n1 RT, we get