Consider the reversible isothermal expansion of an ideal gas in a closed system at two different temperatures T 1 and T 2 T 1 < T 2 . The correct graphical depiction of the dependence of work done w vs the final volume V is:

Step-by-step solution

w = - nRTln ⁡ v 2 v 1 w = - nRTln ⁡ v f v i w = nRTln ⁡ v b v i w = nRT ln ⁡ v f - ln ⁡ v i w = nRTln ⁡ v f - nRTln ⁡ v i y = mx - c So for T 2 > T 1 Intercept of T 2 would be more negative than T 1 and slope of curve T 2 would be more than slope of curve T 1 .