Chemistry Chapter 13

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38 Terms

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Boyle’s Law
P1V1 = P2V2
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Charles’s Law
V1/T1 = V2/T2
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Gay-Lussac’s Law
P1/T1 = P2/T2
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Combined Gas Law
P1V1/T1 = P2V2/T2
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Dalton’s Law of Partial Pressures
Ptotal = P1 + P2 + P3 + P4 + …
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STP atm
1\.00
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STP kPa
101\.325
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STP mmHg/torr
760
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STP temp (K)
273
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Ideal Gas Law
PV = nRT
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Ideal Gas Law + mass and molar mass
PVM = mRT
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density of a gas
m/V
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Avogadro’s Principle
22\.4 L/ mol
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expands
____________ to assume the shape and volume of its container
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flows
readily ____________
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straight lines
particles only move in ____________
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compressible
molecules far apart but ____________
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few
____________ attractive forces between particles
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volume
space occupied by a gas sample
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mL, L, cm^3, dm^3
volume units
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1 cm^3
1 mL = ____________
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1dm^3
1 L = ____________
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temperature
a measure of the average kinetic energy of a group of particles
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thermometer
measurement tool for temperature
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kelvin (K)
temperature unit
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amount
number of moles of the substance
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mol
amount unit
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pressure
force per unit area caused by the collision of the gas molecules with the walls of the container
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manometer
measurement tool for pressure
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pascal (Pa), atmosphere (atm), torr, millimeter of mercury (mmHg)
pressure units
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kinetic molecular theory
a model that uses particle motion and interparticle forces to properties of different states of matter
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no volume
individual gas particles have almost ____________
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inter particle
gas particles have no ____________ forces
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constant random
gas particles are in ____________ motion
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elastic
collisions are ____________, no energy lost
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average kinetic energy
all gases have the same ____________ at a given temperature
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high temp and low pressure
real gases behave like ideal gases at:
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avogadro’s principle
equal volume of all gases measured at the same temperature and pressure contain the same number of particles