Chapter 15 - Ideal Gases Flashcards

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1
Q

Define one mole.

A

6.02x10²³ (Avogadro’s constant) particles of a substance.

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2
Q

What is meant by the phrase ‘ideal gas’?

A

A gas that obeys the three gas laws, Boyle’s Law, The Pressure Law and Charles’ Law.

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3
Q

State Boyle’s Law

A

At a constant temperature, the pressure and volume of a gas are inversely proportional.

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4
Q

State The Pressure Law.

A

At a constant volume, the pressure of a gas is directly proportional to its absolute temperature.

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5
Q

State Charles’ Law.

A

At a constant pressure, the volume of a gas is directly proportional to its absolute temperature.

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6
Q

What do the letters R and n represent in the equation PV = nRT?

A

R = molar gas constant.
n = amount of gas in moles.

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7
Q

What do the letters N and k represent in the equation pV = NkT?

A

N = number of particles.
k = the Boltzman constant.

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8
Q

How do newton’s laws apply to the kinetic theory of gases?

A

-No forces between particles, so they move with constant velocity.
-When a particle collides with a wall, the wall exerts an equal and opposite force on the particle.
-The size of this force can be calculated with F = ma.

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9
Q

Describe pressure using the kinetic theory of gasses.

A

A large number of particles are constantly colliding with the container walls, exerting a steady force.

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10
Q

State the six assumptions of kinetic theory.

A

-The gas contains a large number of particles.
-Particles move rapidly and randomly.
-The volume of particles is negligible compared to the volume of the gas.
-Collisions are perfectly elastic.
-The duration of each collision is negligible.
-No forces between particles.

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11
Q

Why do we use root mean square speed?

A

The average velocities of particles in a gas would amount to 0, so r.m.s. speed is used to give the typical speed.

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12
Q

How do we work out the internal energy of an ideal gas particle?

A

Internal energy = kinetic energy. Potential energy is 0J because there are no forces between particles.

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