Pre-Test Ideal Gas

What is Ideal Gas?

• A gas that obeys the law Pv = NkT

• A gas that obeys the law Pv ~ T

• A gas that obeys the law P ~ vT

• A gas that obeys the law Pv = NRT

What is the SI unit for a given substance?

Hint: _____ is the amount of substance which contains the Avogradro number amount of particles... (5 letters)

How many molecules comprise one mole of a given substance?

One mole of any substance contains Avogadro’s number of constituent molecules: ....​ (a)  

• 6.02 x 10^23 molecules

• 6.02 x 10^22 molecules

• 6.22 x 10^22 molecules

What is the ideal gas equation?

• Pv = NkT

• PV = 1/3Nm(c^2)

• PV = nRT

• PV = 3/2kT

‘All collisions between particles and particles on the wall are elastic’ is an assumption of ideal gas.'

• True

• False

What are the key assumptions in the kinetic theory of gasses? (Choose the appropriate answers)

• Molecules move in random, rapid motion

• Collisions of particles are plastic collisions, Ke1 = Ke2

• Time taken for collisions is negligible/very fast

• Between collisions there are no intermolecular forces between particles

• Gas molecules obey Newton’s laws of gravity

Does increasing the temperature of the balloon while keeping the volume the same increase or decrease the volume on the gas?

• Increase

• Decrease

Use the kinetic theory of gases to explain why a temperature increase would lead to an increase in pressure for a gas that is contained within a container of invariant volume.

• A temperature increase means the particles have more kinetic energy.

• An increase in pressure would mean there are less collisions happening and will have more kinetic energy

• More kinetic energy means a greater change in momentum during collisions with the container. There are also more frequent collisions.

• Change in momentum is proportional to force applied, and therefore to pressure as well.

Assuming constant pressure, how are the volume and temperature of a gas related?​ ​ (a)  

• Directly proportional

• Inversely proportional

What is meant by the root mean square speed?

• The square root of the mean of the squares of the speeds of the molecules.

• The square root of the mean of the speeds of the molecules.

• The square root of the square of the mean of the speeds of the molecules.

• The square root of the square of the speeds of the molecules.