Chapter 7- The Gas Phase
Quiz yourself by thinking what should be in
each of the black spaces below before clicking
on it to display the answer.
Help!
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| The phases/states | solid, liquid, gas
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| Gases | molecules move rapidly, are far apart, can expand to fill any volume, take the shape of a container, and are compressible
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| What variables help define gases | P, V, T, n
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| (STP) P (pressure) | 1 atm = 760 torr = 760 mm Hg
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| V (volume) | mL or L
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| (STP) T (temperature) | 273 K
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| STP | standard temp and pressure = 1 atm and 273K; V = 22.4L, n = 1mole
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| Standard Conditions | 298K, enthalpy, entropy, Gibbs, voltage
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| Ideal Gases | a hypothetical gas whose molecules have no intermolecular forces and occupy no volume; high temp, low P
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| Boyle's Law | Under isothermal conditions, P1V1 = P2V2
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| Charles' Law | under constant pressure conditions, V1/T1 = V2/T2
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| n | number of moles
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| Avogadro's Principle | when pressure and temp are constant, n1/V1 = n2/V2
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| Ideal Gas Law | PV = nRT
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| R | gas constant; = 8.21E-2; 8.314J/Kmol
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| Density | mass/volume; g/L for gases
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| Deviations Due to Pressure | as P increases, gas condenses into liquid state
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| Deviations Due to Temp | As T decreases, gas condenses into liquid state
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| Dalton's Law of Partial Pressures | the total pressure of a gaseous mixture is equal to the sum of the partial pressures of the individual components; Ptot= P1 + P2 + etc
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| P1 = Ptot (X1) | Partial pressure equation
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| KE equation for gases | avg KE is proportional to absolute T; KE = 3/2 KT
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| Graham's Law of Diffusion and Effusion Eq | r1/r2 = [MM2/MM1]^1/2
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