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Chapter 12 Gas Laws

Chloe Hafner & Gunindu Abeysekera
by

Gunindu Abeysekera

on 12 June 2013

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Transcript of Chapter 12 Gas Laws

Chapter 12 Gas Laws
Chloe Hafner
Gunindu Abeysekera

Boyle's Law
Volume
Pressure (kPa)
P
V
Boyle's Example
Remember: P1 x V1 = P2 x V2
The volume of a balloon is 2L; it contains 60 atm of helium pressure in it. What would be the volume of the balloon if the pressure increases to 75 atm?
Charles' Example
V1
T1
=
V2
T2
Remember:
A balloon is filled with 2L of helium and is in an current environment at 283K, when Charles and Carl arrive in Antarctica, they notice the temperature decrease to 253K, also noticing the balloon deflate. What is the NEW volume of the deflated balloon?
Charles' Law
Volume
Temperature (K)
P
V
Gay-Lusaac's Example
The pressure of a balloon is 60 atm and is currently in
an environment at 348K, but when Gay-Lusaac and Carl
arrive in the Sahara desert, the temperature increases to
373K, what is the NEW pressure?
Remember:
P1
T1
=
P2
T2
Gay-Lusaac's Law
Temperature (K)
Pressure
P
V
Dalton’s Law of
Partial Pressures
Calculation of a mixture of gases when the pressure and temperature are constant
Equation: (Just add the pressures of the reactants used)
P(total) = P1 + P2 + P3...
Dalton’s Law of Partial Pressures
Example
The air inside Carl's house is filled with _____ kPa of
helium, 50 kPa of oxygen, and 70 kPa of nitrogen. The total pressure is 150 kPa. What is the partial pressure of helium?
Graham's Laws
tendency of molecules to move from areas of high concentration to areas of low concentration, balancing the concentrations.
Diffusion:
Effusion:
process in which a gas escapes through a tiny hole in a container.
Graham's Law of Effusion/Diffusion
The rate of effusion
of a gas is inversely proportional to to
the square root of a gas' molar mass.
Gases with lower molar mass move faster than gases with higher molar mass.
A balloon filled with helium deflates faster than one filled with air.
Rate A
Rate B
=
Molar Mass B
Molar Mass A
Graham's Example
Remember:
Rate A
Rate B
=
Molar Mass B
Molar Mass A
Compare the rates of effusion of:
Oxyegn (A)
Helium (B)
Full transcript