One mole of an ideal gas is expanded freely and isothermally at 300K from 10 liters to 100 liters. If ΔU=0, the value of ΔH is:
Isothermally at 27∘C, one mole of a Van der Waal's gas expands reversibly from 2 liters to 20 liters. Calculate the work done if a = 1.42 × 1012 dynes cm4 per mole and b = 30 cc
Isothermally at 27∘C, one mole of a vanderwaal's gas expands reversibly from 2 liters to 20 liters. Calculate the work done if a = 1.42 × 1012 dynes cm4 per mole and b = 30 c.c