Kinetic Theory of Gases

According to the kinetic theory of gases, gas particles

• Do not always move in straight lines

• Have most their volume occupied by empty space

• Attract each other

• Do not always move randomly

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NGSS.HS-PS2-1

The kinetic energy of a gas is dependent on temperature

• True

• False

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NGSS.HS-PS3-2

Energy is lost when particles collide with each other or the walls of the container

• True

• False

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NGSS.MS-PS3-5

Gas pressure is caused by

• Molecules colliding with each other

• Molecules condensing to a liquid

• Molecules colliding with the walls of containers

• Barometers

When a balloon filled with air is placed in the freezer, the balloon will

• Expand

• Shrink

• Stay the same size but decrease in temperature

• Stay the same size and temperature

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NGSS.MS-PS1-4

When you push down on a bike tyre, you feel resistance because

• The kinetic energy of the particles increases so the temperature increases

• The kinetic energy of the particles increases so the pressure increases

• The volume has increased so the pressure increases

• The volume has decreased so the pressure increases

Absolute zero is defined as

• O^o Celcius

• O Kelvin

• 273.15^o Celcius

• 273.15 Kelvin

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NGSS.HS-PS3-4

An ideal gas is

• Not a real gas

• A gas that only occurs under certain conditions

• A gas that has particles that are slightly attracted to each other

• A gas that behaves according to the laws of the Kinetic Theory

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NGSS.HS-PS3-2

At 20^oC, the same volume of helium and hydrogen gas will have

• the same average kinetic energy

• the same kinetic energy for all particles

• different kinetic energy as they weigh different amounts

• different kinetic energy as the particles are different sizes

Tags

NGSS.HS-PS3-2