3.6 Deviation from Ideal Gas Law

Does the ideal gas law explain actual behavior of real gases?

No

Deviations from the ideal gas law may result from:

Interparticle attractions among gas molecules and particle volumes

Deviations from ideal gas law in terms of interparticle attractions among gas molecules occur particularly at conditions that are:

Close to those resulting in condensation

Deviations from ideal gas law in terms of particle volumes occur particularly at:

Extremely high pressures

In an ideal gas, it is assumed that there are ______ between the gas particles

No attractive forces

Do particles of a real gas experience attractive forces?

Yes

The effect of real gas having attractive forces is especially noticeable when the gas temperature is relatively:

Low

The attractive forces between gas particles can increases/decreases the force with which the particles collide with the container walls

Decrease

If the force with which the particles collide with the container walls is decreased, the observed pressure of the gas is greater/lesser than the value predicted by the ideal gas law

Lesser

In an ideal gas, it is assumed that the volume occupied by the gas particles themselves is:

Zero or negligible

In an ideal gas, it is assumed that the free space in which the gas particles can move around is equal to the:

Entire volume of the container

Do particles of a real gas have volume?

Yes

Do particles of a real gas occupy space inside the container?

Yes

The effect of gas particles occupying space inside the container is especially noticeable when the gas pressure is very:

High

When the volume of the gas particles themselves becomes a significant fraction of the container volume, the free space in which the particles can move around is increased/decreased

Decreased

When the free space in which gas particles can move around is decreased. the observed pressure of a real gas is greater/lesser than the value predicted by the ideal gas law

Greater

A gas sample exhibits ideal behavior at relative high/low temperatures and high/low pressures

High; low