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760 mmHg
760 Torr
1.01325 Pascals
101.325 Kilopascals |
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1kg/m*s2
SI unit of pressure |
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1)open manometer= pgas=patm+deltahHg
2)closed manometer=pgas=deltah |
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Pressure and Volume are inversely proportional
~as pressure increases, volume decreses |
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Volume and Temperature are proportional
~as volume increases, temperature increases |
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Moles and Volume are proportional
~as # of moles increases, volume increases |
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Pressure and Temperature are proportional
~as pressure increases, temperature increases |
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| P1V1/n1T1=P2V2/n2T2; where n is constant |
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| Volume occupied by 1 mole of gas at STP; 22.4L |
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| Calculating Density of a gas at STP |
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Definition
Divide it's molar mass by it's molar volume
1)d=m/v=PM/RT |
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Patm=P1+P2+P3...etc...etc
the total pressure of any mixture of gasses equals the sum of all the partial pressures of the gases in the mixture |
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| moles of a substance/total moles in mixture |
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1)gas molecules have tiny volumes compared with the collective volume they occupy (no volume is assumed)
2)they move constantly and randomly
3)the motion of these molecules is associated with an average kinetic energy proportional to the absolute temperature of the gas
4)They continually collide with eachother and these collisons are elastic
5)There are no attraction or repulsion forces acting on these molecules |
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| urms=the square root of (3RT/Molar mass) |
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| rsubx/rsuby=square root of (molar mass x/molar mass y) |
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| Gas escapes from it's container through a tiny hole into a region of lower pressure |
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| The spread of one substance (usually a gas or liquid) through another |
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| van der Waals equation for real gases |
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