Transcript Ideal Gas Law

Ideal Gas Law

k1
P
V


V = k 2T
V = k 3n

PV = (k1k2k3)nT
PV = k1
PV = nRT
Ideal Gas Constant
L  at m
R  0.0821
mol K
L  kP a
R  8.31
mol K

Example
How many moles of gas would be in a 500. mL
bottle at 2.3 atm and 295 K?
1L
500. mL 
 0.500 L
1000 mL
PV=nRT
(2.3 atm)(0.500 L) = n(0.0821
L  atm
mol  K

2.3 atm0.500L 
n
L  atm 

 0.0821
295 K 

n = 0.047 mol
mol K 
)(295 K)

What volume does 4.24 g of nitrogen gas
occupy at 58.2oC and 2.04 atm?
1 mol
4.24 g N 2 
 0.151 mol N 2
28.02 g
58.2oC + 273.15 = 331.4 K
PV=nRT
L  atm
(2.04 atm)V=(0.151 mol)(0.0821mol  K )(331.4 K)
V = 2.01 L