what is the pressure of a mixture of helium, nitrogen, and oxygen...?
821966
Not sure where the 600 came from, but it sounds like the question wants the total pressure of all the gases combined.  So you would just add together all the partial pressures, and the total pressure is 330 mm Hg.\n\nDividing the total pressure by the number of gases would give you the average partial pressure, but I don't think that's very useful.
53064
Assuming your gas is an ideal gas, you can use the ideal gas law.\n\nPV=nRT where \nP=Pressure in atm (1 atm= 760 mm Hg so 730 mm Hg= 0.96atm\nV=volume in L\nn= moles\nT=Temperature in K (C=K+273 so 30 C = 303 K)\nR= the universal gas constant= 0.08206 L-atm/mol-K\n\nSolve the ideal gas equation for n=PV/RT\n\nn=[(.96atm)(10L)]/[(.08206 L-atm/mol-K)(303K)]\n\nn=0.386 moles
497026
Lol, trying to get people to do your chemistry homework?\nUse PV=NRT \nP = Pressure in ATM (1 ATM in STP)\nV = Volume in liters (convert 65cc to liters)\nN = number of moles (will be constant)\nR = gas constant (0.0821 L.ATM/ Mol.K)\nT = temp in Kelvin (273 + degrees C) (STP = 273 K or 0 C)\n\nwith moles being held constant, and the gas constant being constant, your equation should look like;\n\nPV/T (initial) = PV/T (final). solve for P (final)\n\nIf you can't solve this in an hour, i'll post the answer.\n\n....... i was hoping you'd try to solve this and post your answer.....\n\ni got .9383 ATM as the new pressure. mind, that answer is not in sig fig.
787380
PV=nRT\nP=pressure\nV=volume\nn=moles\nR=constant(.08026atm*L/mol*K)\nT=temperature\n\nThis is the ideal gas law.
650823
Carbon, Hydrogen, and Oxygen.
814078
Pressure and volume are inverses of each other and therefore you can't in the first place say they are at constant pressure unless they were in the same container (When they do mix).. so when they are separated, you can't have the same pressure at different volumes. Though your experiment shows the achievement of equilibrium of high to low pressure, as the bigger one gets bigger (right?)...\n\nAnyways, finding an inexpensive experiment (on the web) is really difficult.  Dalton's law can be used as you probably know by collecting water over gases (which requires some lab equipment and some chemicals not readily available so to say) and also has an application in scuba diving.  I'll ask someone for you that I know... Can you give me 'till Monday or Tuesday to get a good answer for this or when does your presentation have to be done?
386823
There is some 02, N2, CO2. There are also a daub of Argon, hydrogen, neon, helium, and a couple of others I don't remember.\n\nAs a matter of interest, more commercial plants that product liquid nitrogen, oxygen etc, start with liquidfied air and then separate the various components.
635000
The easiest way to work this out is from the Ideal Gas Law, PV=nRT. Assuming that they start at the same temperature, this is even easier because both R and T will be constants.\n\nLets make the first gas 1, the second gas 2 and the final mix f so that :\n\nPressure Gas 1 =P1, Volume Gas 1 = V1, Temperature Gas 1 = T1\nPressure Gas 2 =P2, Volume Gas 2 = V2, Temperature Gas 2 = T2\nPressure final mix =Pf, Volume final mix = Vf, Temperature final mix = Tf\n\nthen :  P1V1/RT1+P2V2/RT2=PfVf/RTf\n\ntake out the constant R\n\nP1V1/T1+P2V2/T2=PfVf/Tf\n\nIf T is different for each mix\n\nPf=(Tf*(P1V1/T1+P2V2/T2))/Vf\n\nif T is constant (which I assume from your question)\n\nP1V1+P2V2=PfVf\n\nPf=(P1V1+P2V2)/Vf\n\nOkay?
430954
A number of differnt elements, including oxygen, hydrogen, nitrogen, carbon, argon and others.  The mojority of air is nitrogen at about 63%, while depending where int he world you are, oxygen only makes up 15-19 percent.
1103330
My thought is air as well. Air is composed of around 2/3s part of Nitrogen. Oxygen is a much smaller amount
247481
If I'm not mistaken, they will have the same pressure, as they are in equal number of molecules. 17grams of Amonia or NH3 sum up 1mol of NH3 molecules while 2 grams of Hydrogen, H2 consists of 1mol of Hydrogen molecules. \nAn equation : Pv = nrT, where P= pressure, v=volume, n is the number of molecule/atom, r is a constant, and T is the absolute temperature (in Kelvin). Since they are equal in their number of molecules, it share the same pressure. Hope it helps.
695888
I assume the temperature is high enough that the O2 & Ne behave as ideal gases.\n\nThe partial pressure of each gas in a mixture of gases is proportional to its mole fraction.\n\nMoles of Ne = 12.6/20.18 = 0.6244\nMoles of O2 = 7.10/32.00 = 0.2219\nTotal moles = 0.6244 + 0.2219 = 0.8463\nMole fraction of Ne = 0.6244/0.8463 = 0.7378\nPartial pressure of Ne = 0.7378*0.435 = 0.321 atm (answer)\nMole fraction of O2 = 0.2219/0.8463 = 0.2622\nPartial pressure of O2 = 0.2622*0.435 = 0.114 atm\nTo check to make sure there are no errors:  0.114 + 0.321 = 0.435
540399
hey! Air is a mixture of gases thus it is solution, it contains Nitrogen-78%, oxygen-20.9% carbon dioxide0.003% and some rare gases
912161
Nitrogen (N2) 780,840 ppmv (78.084%) \nOxygen (O2) 209,460 ppmv (20.946%)
987167
Atmospheric pressure and physics
103755
it is a mixture not technically a solution. now if you are diving deep they mix nitrogen, oxygen, and hellium. i think it's called "trimax" i could be wrong about that name. the hellium helps keep your vision clear at deeper depths.
716268
PV = nRT\nn = PV/RT\n\nP = standard pressure(don't know which one you're picking)\nV = 2 L\nT = standard temp(again don't know which one you're picking)\nR = constant you can decide which one you want to use at\nhttp://en.wikipedia.org/wiki/Ideal_gas_constant