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28 Cards in this Set
- Front
- Back
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pressure =
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force
------- area |
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Gas pressure depends on:
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how often collisions occur per area and how hard they strike.
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more collisions =
harder strike = |
more collisions = more pressure
harder strike = more pressure |
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The pressure exerted on Earth by its atmosphere:
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Atmospheric pressure
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Instrument that measures atmospheric pressure:
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Barometer
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SI unit of pressure:
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1 pascal (Pa)
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1 atm =
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760mmHg = 760torr = 101,325 Pa = 14.7psi
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Gas temps. are always calculated in:
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Kelvin
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TK = t˚C +
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273.15
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KE =
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1/2mv²
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Describe the properties of gasses:
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-particles are in constant random motion
-there are no attractive or repulsive forces between particles. -Particles can collide without losing energy -Particle speed increases with temp. increase. |
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Boyle's law =
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P₁V₁ = P₂V₂ constant T and quantity.
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Multiple gasses mix..
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evenly and completely and exert a uniform pressure.
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Charle's Law
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V₁/T₁ = V₂/T₂
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Combined Gas Law is a combination of:
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Boyle's Law and Charles Law
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Combined Gas Law
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P₁V₁/T₁ = P₂V₂/T₂ Quantity must be constant.
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Avagadro's Law
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V₁/n₁ = V₂/n₂
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Avagadro's Law states that:
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Equal volumes of any two gases contain equal # of particles and equal # of moles.
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STP =
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0˚C and 1atm
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Standard Molar Volume =
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22.4 L at STP
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The Ideal Gas Equation is:
R = |
PV = nRT
R = 0.08206 L*atm / mol*K |
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The ideal gas equation combines these laws:
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Boyle's, Charle's, and Avagadro's gas laws.
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Partial pressure:
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the pressure exerted by a gas in a mixture.
-same pressure the gas would exert alone. |
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Dalton's Law of partial pressures:
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Total pressure of mixture of gases is the sum of the partial pressures.
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Dalton's Law
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Ptotal = P₁ + P₂ + P₃ +
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1L = __dm³
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1L = 1dm³
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1mL = __cm³
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1mL = 1cm³
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__L= M³
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1000L = M³
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