Chem 172 - Ch 10 equations / equivalent conversions

pressure in the case of force applied to an area

P = F/A

1 Pa is equal to

1 N / m² is equal to

1 bar is equal to

10^5 Pa

1.00 atm is equal to

760 torr is equal to

values for STP

T - 273 K or 0 degrees C

P - 1.00 atm

760 torr or 1 atm is equal to

101.325 kPa is equal to

Boyles’s Law

P = c/v to P1 V1 = P2 V2

Charles’ Law

c = V/T to V1 / T1 = V2 / T2

Avogadro’s Law

v= cN to V1 / n1 = V2 / n2

ideal gas equation

PV=nRT

ideal gas assumptions

- no attractive forces

- neglect particle volume

- there is identical molar volume at STP no matter the gas ID

- the gas consists of individual point particles

density of ideal gas formula

d= PM / RT

Dalton’s Law of Partial Pressures

P1 = n1 / nT times Pt

Dalton’s Law of Partial Pressures important notice

the total pressure of a mixture of gases equals the sum of the partial pressures that each would exert if present alone

kinetic molecular theory

1) gases consists of large numbers of molecules that are in continuous, random motion

2) the combined volume of all the molecules of the gas is negligible relative to the total volume in which the gas is contained

3) no attractive forces

4) average kinetic energy depends only on absolute temp

effusion

the escape of gas molecules through a tiny hole into an evacuated space

diffusion

the spread of one substance throughout a space or throughout a second substance

deviations from ideal gas behavior

assumptions made in KE molecular theory don’t hold true if there is high pressure and / or low temperature

real gases behavior

most ideal behavior is a higher temperature (1000K) and the molecules have lower average KE so the attractive forces can take over

van der Waals equation

(P+n²a/v²) (V-nb) = nRT