3/9/2012
Combined Gas Law
Combined Gas Law
P1V1 = P2V2
T1
T2
A sample of diborane gas, B2H6, a substance that bursts
into flame when exposed to air, has a P of 345 torr at a T
of -15C and a V of 3.48 L. If conditions are change such
that the T is 36C and the P is 0.616 atm, what will be the
V?
1
3/9/2012
Ideal Gas Law
• PV=nRT
• n = number of moles
• Universal gas constant
R = 0.08206 L atm/K mol
Units for variables MUST match those in the
gas constant
The Ideal Gas Law
• PV=nRT
n=# of moles
R = 0.08206 L atm/K mol
How many moles of Argon gas can be found in a
cylindrical light tube with a volume of 3.7 L and a
under a pressure of 162 KPa. The T in the tube is 350 K.
2
3/9/2012
• PV= g (R)(T)
FM
How many grams of carbon dioxide are in your lungs at a
T of 37C and under a pressure of 768 mmHg. Your lung
capacity is 4.8 L.
Finding density
• PFM = g = d
RT
V
Calculate the density of NO2 at 300K if its under a
pressure of 6 atm in a 5.0 L container.
3