The ideal had law assumes no molecular volume and no intermolecular forces. in actuality real gases exhibit both. assume a typical unknown gas had a mass of 0.300g and a density at room temperature of 0.79 g/ml. also assume the measured volume of the flask was 265.4ml. what is the actual volume for the gas molecules to move about in the flask?

The actual of gas is 0.38 mL when it put into the 265.4 mL flask it expand and occupy all available volume.

Explanation:

Given data:

Mass of gas = 0.300 g

Density of gas = 0.79 g/mL

Volume of flask = 265.4 mL

Volume of gas = ?

Solution:

Formula:

D=m/v

D= density

m=mass

V=volume

v = m/d

v = 0.300 g/ 0.79 g/mL

v = 0.38 mL

The actual of gas is 0.38 mL when it put into the 265.4 mL flask it expand and occupy all available volume.