12.5 mol of a gas occupies a volume of 275 cm3 at 90.0 atm. Use the reduced van der Waals’ equation to obtain the temperature of the gas, given that the critical molar volume, temperature and pressure are 59.1cm3 mol–¹, 647K and 218.3 atm respectively?

Virtuestar

4 years ago

In chemistry and thermodynamics, the Van der Waals equation (or Van der Waals equation of state) is an equation of state which extends the ideal gas law to include the effects of interaction between molecules of a gas, as well as accounting for the finite size of the molecules. The ideal gas law treats gas molecules as point particles that interact with their containers but not each other, meaning they neither take up space nor change kinetic energy during collisions (i.e. all collisions are perfectly elastic). The ideal gas law states that the volume V occupied by n moles of any gas has a pressure P at temperature T given by the following relationship, where R is the gas constant: PV=nRT