Gas Laws Practice Quiz

Gas molecules exert pressure on the walls of the container because of

• momentum

• they obey gas laws

• they collide with each other

• they have finite volume

Pressure is caused by

• gravity

• gas molecules colliding with each other

• gas molecules colliding with surface

• gas molecules reacting with each other

Which of the following statement(s) is/are true.

• The molecules in a gas take up a negligible amount of space in relation to the container they occupy.

• No energy is gained or lost when molecules collide.

• The molecules are in constant, linear motion.

• All are true

Which one of the following is not a statement of kinetic theory of gases?

• The KE depends upon the temperature of the gas

• The KE depends upon the pressure of gas

• The collisions are elastic

• Pressure of gas is due to collisions of gas molecules on the walls of the container

According to kinetic theory of gases, the collisions between molecules of a gas:

• occur in a zig-zag path

• occur in a straight line

• change velocity and energy

• result in settling down of molecules

Particles will experience large velocities at ...

• Low temperature

• Intermediate temperature

• High temperature

• All of the above

Each of the containers is shown at the same temperature. In which container is the average speed of the particles the fastest?

• chlorine

• nitrogen

• hydrogen

• oxygen

In an ideal gas, if everything else is held constant, tripling the pressure will ________ the Kelvin temperature.

• triple

• cut into a third

• not affect

• equal

Answer explanation

$PV=nRT$

If you multiply P by 3, you would have to multiply T by 3 as well in order to keep the right side equal to the left.

In an ideal gas, if everything else is held constant, doubling the volume will ________ the pressure.

• double

• halve

• not affect

• eliminate

Answer explanation

$PV=nRT$

Since nRT cannot change, neither can PV. If you multiply V by 2, you would have to multiply P by 1/2 to keep the right side constant.

According to kinetic molecular theory: at constant temperature, increasing the volume will decrease the pressure because...

• the gas particles must travel farther from wall to wall.

• P and V are on the same side of the ideal gas law equation.

• the average velocity of the gas particles decreases.

• the potential energy of the gas particles has gone down

Answer explanation

farther travel = fewer collisions per second

In kinetic molecular theory:

pressure = collisions per second between gas and walls of container

temperature = average kinetic energy of gas molecules (as measured by temperature)