Term
| Units of Measurement for Gases |
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Definition
same units as volume:
ml,cc,cm3, L |
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Term
| Temperature Units of Gases |
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Definition
gases must be measured in Kalvin:
C-K= C+ 273
F-K= [(F+40)5/9]-40+273 |
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Term
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Definition
| occurs at 0 K; all molecular motion ceases |
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Term
| STP(Standard Temperate Pressure) Conditions |
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Definition
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Term
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Definition
| atmosphere(atm), milimeters of mercury(mmHg/torr), pounds per in2(psi), kilopascals/kilopaskals(Kpa) |
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Term
| Pressure Unit Conversions |
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Definition
| 1 atm=760 mmHg/torr=14.7 psi=101.3 Kpa |
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Term
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Definition
| defines as force per unit area : P=F/A |
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Term
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Definition
| pressure that is exerted by the gas molecules in Earth's atmosphere on its surface |
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Term
| Dalton's Law of Partial Pressures |
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Definition
| total pressures in any enclosed system is = to the total sum of the partial pressures (Pt=P1+P2+P3...Pn) |
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Term
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Definition
| explains gas behaviors in terms of molecular motion and distance |
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Term
| Four Basic Postulates of KMT |
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Definition
1) gas molecules are spaces far apart; gases are mostly empty space
2)gas molecules are in continuous, rapid, and linear motion(average speed of a gas molecule is 1000m/s)
3)pressure exerted by gases is a result of collision of gases(these are perfectly elastic) and no energy is lost
4) increase in temperature will increase the speed of gas molecules |
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Term
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Definition
P1*V1=P2*V2(temperature is the constant variable)
*pressure is inversely proportional to volume |
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Term
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Definition
V1/T1=V2/T2( pressure is the constant variable)
*volume ans temperature are directly proportional |
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Term
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Definition
P1/T1=P2/T2(volume is the constant variable)
*pressure and temperature are directly porportional |
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Term
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Definition
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Term
| Molecular Volume of Gases |
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Definition
*at constant temperature and pressure the volume is proportional to the mass
* molar volume is = to molar mass/density[(g/mole)/(g/)=L/mole
* all gases at the same temperature& pressure have the same molar volume
*molecular masses of 2 gases are in the same ratio as their densities (mm1/mm2=d1/d2) |
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Term
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Definition
| 1 mol of any gas under STP conditions will occupy a vol of 22.4L/mole |
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Term
| Ideal Gas Law(used when conditions are unchanging) |
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Definition
| *assumes vol is proportional to the # of mols, absolute temp; is inversely proportional to pressure |
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Term
| PV=nRT(ideal gas aw equation) |
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Definition
| P=pressure(atm), V=volume(L), n=# of mols, T=temperature(K), R= gas constant(0.0821) |
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Term
| PVM=gRT(alternate for ideal gas law equation) |
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Definition
| *n is substituted by g/M(g=total mass of sample, M=molecular mass) |
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Term
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Definition
| gases behave ideally at high pressure conditions and low temperature conditions |
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Term
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Definition
| volume ratio is = to the mole ratio in a balanced chemical equation |
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