Gas Laws and Kinetic Molecular Theory

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

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.HS-PS3-4

Gas pressure is caused by

• Molecules colliding with each other

• Molecules condensing to a liquid

• Molecules colliding with the walls of containers

• Barometers

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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

NGSS.MS-PS3-4

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

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NGSS.HS-PS2-1

Which of the following is not an assumption of kinetic theory of gases?

• the total volume of the particles are negligible compare to the volume of container

• the number of particles are large

• the particles are moving with the same speed

• the collisions of particles are elastic

State what is meant by the internal energy of a matter.

• it is the sum of kinetic energy of the particles.

• it is the sum of potential energy of the particles.

• it is the sum of kinetic and potential energy of the particles in random motion.

• it is the ratio of kinetic to potential energy of the particles.

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• the number of molecules in unit volume of the gas

• the total number of molecules in one mole of gas

• the total number of molecules  present in volume V

• the mass of gas present in volume V

• the average of the squares of the speeds of the gas molecules

• the root-mean-square of the gas molecules

• the square of the average speed of the gas molecules

• the sum of the squares of the speeds of the gas molecules