CHEM1011 Lecture Notes - Lecture 5: Diffraction, Refraction, Mole Fraction
CHEM1011 – Chemistry 1A – Part 3
LEC 5: *Continued
o Manometer: measure differences in pressure of two gases
• Gas density:
m = mass (g), v = volume (L)
• Using density in the ideal gas equation:
M = Molar mass, P = pressure, R = constant, T = temp.
• Find molar mass from the density of a gas:
LEC 6: Partial pressures, effusion and diffusion
Theory
• Partial pressures: Partial pressure of a gas in a mixture is its mole fraction x total
pressure. Ptotal = P1 + P2
• Partial pressures are based on the assumption that in a mixture of gases, the total
pressure exerted is the sum of the partial pressures that each gas would exert if it
were alone under the same conditions.
• Mole fraction:
• Rate of gas movement:
• Graha’s Law of effusio: Rate of effusion (gas escaping into a vacuum)
o Higher the molar mass, the slower the gas will effuse.
• Rate of diffusion (movement of one gas through another)
• If equal pressures of gases are known and the rate of diffusion of one gas is known, it
can be used to calculate the rate of the other gas.
o
or
LEC 7: Atomic Structure
Theory
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