DAT chem 4 - GASES

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Last updated 5:50 AM on 5/21/26
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20 Terms

1
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Do gasses have definite volume

No, like liquids, they fill the container they are in, but unlike liquids, they do not have a definite volume

<p>No, like liquids, they fill the container they are in, but unlike liquids, they do not have a definite volume </p>
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SI unit for volume

liter, 1 liter is equal to 1 cm³

<p>liter, 1 liter is equal to 1 cm³</p>
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Pressure formula

force/area

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Pressure units

1 atm = 760 torr = 760 mmhg

<p>1 atm = 760 torr = 760 mmhg</p>
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What is an ideal gas

a gas that can be explained using the ideal gas law

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Under what condtions is a gas ideal?

at high temp and low pressure

<p>at high temp and low pressure </p>
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Ideal gass assumptions

  1. the volume of a gas particle is insignificant compared to the space between them

  2. gases expierience zero intermolecular forces between them and their containers

  3. Gases are always in random motion

  4. they are perfectly elastic, so there is zero KE loss or gain when they collide with each other

  5. the avg KE of a gas depends on the temp of the system

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Boyle’s law

volume is inversely proportional to pressure

<p>volume is inversely proportional to pressure</p>
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Charle’s law

Volume is proportional to temperature

<p>Volume is proportional to temperature</p>
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Avogadro’s law

Volume is proportional to gas moles

<p>Volume is proportional to gas moles</p>
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Combined gas law

(P1V1)/(T1n1) = (P2V2)/(T2n2)

<p>(P<sub>1</sub>V<sub>1</sub>)/(T<sub>1</sub>n<sub>1</sub>) = (P<sub>2</sub>V<sub>2</sub>)/(T<sub>2</sub>n<sub>2</sub>) </p>
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Ideal gas law

PV=nRT

<p>PV=nRT</p>
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ideal gas constant

0.0821 L*atm/mol*K

<p>0.0821 L*atm/mol*K</p>
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STP

273 kelvin and 1 atm (760 torr, 760 mmhg)

<p>273 kelvin and 1 atm (760 torr, 760 mmhg)</p>
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how much is one mol of gas at STP

1 mole of gas = 22.4L

<p>1 mole of gas = 22.4L</p>
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density formula

mass/volume

<p>mass/volume</p>
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Density for gasses formula

density = (P*molar mass)/RT

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Daltons law of partial pressures

Total pressure inside a container with multiple gases is equal to the sum of the pressures

<p>Total pressure inside a container with multiple gases is equal to the sum of the pressures</p>
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Graham’s law of effusion

when esccaping through a narrow slit, lighter gasses effuse (escape) faster than heavier gasses

due to the fact that KE = ½ mass * velocity²

The lighter ones move faster, as they have the same average KE due to being the same temp

<p>when esccaping through a narrow slit, lighter gasses effuse (escape) faster than heavier gasses</p><p></p><p>due to the fact that KE = ½ mass * velocity²</p><p>The lighter ones move faster, as they have the same average KE due to being the same temp</p>
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Graham’s law of effusion formula

Rate 1/rate 2 = Sqrt(Molecular weight 2/Molecular weight 1)

<p>Rate 1/rate 2 = Sqrt(Molecular weight 2/Molecular weight 1)</p>