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Eng0013 > Ideal Gases and Kinetic Theory > Flashcards

Ideal Gases and Kinetic Theory Flashcards

1
Q

What is the equation for Pressure?

A

Force / Area

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2
Q

What are the three ways to change the pressure?

A

Change number of particles
Change kinetic energy of particles
Change volume of container

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3
Q

Isochoric

A

Constant Volume

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4
Q

Isobaric

A

Constant Pressure

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5
Q

Isothermal

A

Constant Temperature

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6
Q

Adiabatic

A

No heat transfer

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7
Q

Closed System

A

Constant Mass

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8
Q

What is Boyle’s Law

A

For a closed system and a constant temperature the Pressure and Volume are inversely proportional
PV = Const

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9
Q

What is Charles’s Law

A

For a closed system with constant pressure the Volume is proportional to the absolute Temperature
V/T = Const

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10
Q

What is the pressure Law?

A

For a closed system at a constant volume the Pressure is directly proportional to its absolute temperature
P/T = Const

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11
Q

Avogadro’s Law

A

Volume is directly proportional to number of molecules present for a fixed pressure and temperature
V/N = Const

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12
Q

What is Avogadro’s Constant

A

Na = 6.02x10^23

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13
Q

What is the equation for number of particles?

A

No of Mols (n) x Avogadros Constant
N = n x Na

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14
Q

What is Boltzmann’s Constant

A

K = 1.38x10^-23

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15
Q

What are the Ideal Gas Law equations?

A

PV = NKT
PV=nRT
Where n is the number of mols, R is the molar gas constant and N is the number of Particles
R = 8.31

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16
Q

How to calculate work done by a gas?

A

W = p x change in V
Area under the PV graph

17
Q

Equation to calculate mass with ideal gas law?

A

Mr x PV/RT

18
Q

Equation to calculate density with ideal gas law?

A

Mr x P/RT

19
Q

What are the assumptions of an ideal gas?

A

Collisions are instantaneous
Lack of Attraction
Point Masses
Elastic Collision
Random Motion

20
Q

What equation connects the ideal gas equation and kinetic theory?

A

PV = 1/3 Nm(Crms)^2

21
Q

What is the equation for the kinetic energy of ideal gas molecules?

A

1/2m(Crms)^2
3/2nRT/N

Eng0013 (13 decks)

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