|Jun26-11, 10:41 AM||#1|
In a spherical vessel with a hydrogen H2 and oxygen mixture O2 it is stated in a problem that we can derive that the concentration of oxygen [O2] can be derived to be:
P / 3RT. With P the total pressure, R the gas constant en T temperature?
How on earth is this possible? I thought the ideal gas law stated that p = n R T (with n the concentration per unit volume). Any help?
|Jun27-11, 07:52 AM||#2|
See if you can rearrange the general equation, n = PV/RT into a concentration (moles per liter), concentration = P/3RT. If the general gas law only defines the system for all gases, where does that '3' come from?
|concentration, gas law, oxygen, pressure|
|Similar Threads for: Oxygen pressure|
|Oxygen Partial Pressure||General Physics||6|
|Partial pressure of oxygen during Al deposition||Advanced Physics Homework||0|
|Oxygen Tank Problem/Ideal Gas Law - solving for pressure||Introductory Physics Homework||0|
|Initial Mass of Oxygen + Mass of Oxygen leaked out||Introductory Physics Homework||3|
|High pressure oxygen||Quantum Physics||0|