Exam 2 Content (Feb 14th)

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1

For Kinetic-Molecular Theory of Gases what do we assume?

  • gas particles are small relative to the distance between them

  • forces between particles are negilbe expect during collisions

  • between collisions, particles move in straight lines at various speeds

  • collisions are elastic with no loss in keltic energy

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2

What’s diffusion?

movement are particles from higher concentration to low concentration

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3

what’s effusion?

the escape of gas particles through a small opening in containers

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4

lighter molecules collide more frequently in a container thus,

they will effuse faster than heavier ones

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5

heavy molecules collide not as frequent in a contain thus,

they will effuse slower than lighter ones.

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6

What is the rate of effusion?

Urms = 1/ sqrt(molar mass)

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7
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8
<p>What does each part of this equation mean?</p>

What does each part of this equation mean?

Ave.KE → average kinetic engird of the molecules

Mm → molar mass in kg/mol

u² → average rms speed

R → Ideal gas constant

T → temp in Kelvin

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9

if particles are moving slow the temperature will be?

colder

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10

if particles are moving fast the temperture will be?

hotter

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11

as volume increases pressure will?

decrease

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12

as temp goes up, volume will?

go up but pressure will remain the same.

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13

as temp goes down, volume will?

go down but pressure will remain the same

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