Units
5.5 mmHg in torr
5.5 torr
Avogadro's Law
v1/n1= v2/n2
1 atm in torr
760 torr
Grahams Law of Effusion
rate a/ rate b = sqrt( Mb)/ sqrt (Ma)
@ STP
1 mol = 22.4 L
Combined Gas Law
P1V1/T1= P2V2/T2
1 atm in Psi
14.7psi
At constant pressure and moles, a sample of gas has a volume of 0.543 mL at 310K. What is the new volume at 75C?
0.609 mL
What is the volume of 22.1 g of Ne at 55oC at a pressure of 221,345 Pa?
v= 13.6 L
A 12.5-L scuba diving tank contains a helium–oxygen (heliox) mixture made up of 24.2 g of He and 4.32 g of O2 at 298 K. Calculate the mole fraction and partial pressure of each component in the mixture and the total pressure of the mixture.
P He= 11.8 atm
P O2= 0.264 atm
Urms
Urms= sqrt(3RT/M)
1 atm in Pa and Kpa
101.3 kPa
101,325 Pa
A sample of gas at 5.42 atm, 4.2L, and 321 K was increased to a temperature of 162C and the pressure was decreased to 2941.2 mmHg. What is the new volume in mL?
8080 mL
How many moles of a gas are in a system with a pressure of 22.1 psi, a volume of 2.19 L at 34oC?
n= 0.130 mol
A gas mixture contains 0.70 mol of N2, 0.20 mol of H2, and 0.10 mol of CH4. What is the mole fraction of H2 in the mixture? Calculate the pressure of the gas mixture and the partial pressure of each constituent gas if the mixture is in a 10.0 L vessel at 27 C
Ptot= 2.46 atm
PH2= 0.492 atm
PN2= 1.722 atmPCH4= 0.246 atm
Ideal Gas Law and Units
Pv=nRT
p- atm
v- L
n-mol
R- 0.08206 l*atm/mol*k
T- Kelvin