Question

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?

Answer 1

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

Step-by-step 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.