The Gas Phase Flashcards
Four Gas Variables
- Pressure (P)
- Temperature (T)
- Volume (V)
- Number of moles (n)
Unit(s) of Pressure
Pressure = atm, mmHg, torr, kPa
Note:
[1 atm = 760 mmHg = 760 torr = 101.325 kPa]
Unit(s) of Temperature
Temperature = K
Note:
273 + C = K
K - 273 = C
Unit(s) of Volume
Volume = L or mL
Note:
1 L = 1000 mL or 1 x 10^3
Standard Temperature and Pressure
STP = 273 K (0 C) @ 1 atm
Used for Gas Law Equations
Note:
@ STP 1 mole of ideal gas = 22.4 L
Ideal Gas
A hypothetical gas where molecules do not exert intermolecular forces and do not occupy any volume.
Ideal Gas Law
Def.) Describes relationship between P, T, V, and n.
Eq.) PV = nRT
R = 8.314 when P = kPa R = 8.21E^-2 when P = atm R = 62.4 when P = mmHg
Ideal Gas Law: Solve for Pressure (P)
P = nRT/V
Ideal Gas Law: Solve for Volume (V)
V = nRT/P
Ideal Gas Law: Solve for Number of Molecules (n)
n = PV/RT
Ideal Gas Law: Solve for Temperature (T)
T = PV/nR
Ideal Gas Law: Density
d = PM/RT
Note:
d = density
M = molecular weight
Combined Gas Law
[P1V1/T1] = [P2V2/T2]
Avogadro’s Principle
P and T held constant; shows n and V are directly proportional
n/V = k n1/V1 = n2/V2
Note:
- increase in n = increase in V
- decrease in n = decrease in V
Boyle’s Law
T and n held constant; shows P and V are inversely proportional
PV = k P1V1 = P2V2
Note:
- increase in P = decrease in V
- decrease in P = increase in V