What is the measured pressure (P meas)?
821342
THe VdW equation is P= nRT/(V-nb) - a(n/V)^2, just plug and chug.  But dont forget to switch your T into Kalvin
911852
Pressure is nothing but a force applied onto an area. Pressure in air filled balloon, for example,  is due to "concurrent forces" created by compressed air pushing outward from the center on the balloon. These forces are equal in strength that at the center they clear each other. Thus at the center the pressure is a nonsatble 0.
227415
actual pressure of the vapour\ndivided by\nthe maximum pressure of the vapour at 'that' temperature\nequals (in this case) 1 = 100%
851431
MASS / VOLUME\n that's way you measure it in g/mL
552193
Can be solved by simply plugging values into the Ideal Gas equation without using two states.  Pressure must be converted to atmospheres, however, and temperature to Kelvin.  P = 1.243 atm, T = 306 K\n\nn = PV/RT = 1.243 * 2.74 / (0.08206 * 306) = 0.136 mol\n\nmass = moles * MM = 0.136 * 28.01 = 3.81 g
840037
PV = NRT\n\nN - Mols of argon\n\nR = .0821\n T = 26+273.15\n\nV  = 75/1000 to convert to L\n\nThen you will find your P, pressure, in atmospheres.\n\nconvert that to torr
631138
Water pressure is the force exerted by water on its surroundings.\n\nOne example is diving under water. At the surface, the air pressure is one atmosphere (atmosphere is a unit of pressure). If you dive 33 feet down, then the pressure is 2 atmospheres. 66 feet is 3 atmospheres, etc. This means, under 33 feet of water, the force exerted on you by the water is double the pressure of air at the surface (which you don't notice because you're used to it ... you only notice when it changes, such as when you go in an airplane and your ears pop).\n\nAnother example is in pipes. Water is pressurized so that it will flow out of your faucet when you open the tap. The air pressure at your sink is one atmosphere. As long as the water in the pipes is pressurized more than one atmosphere, water will flow when you open the tap.
709574
I get 1.69522 g/L, using constants with the most significant figures I can find:\n\nN/V = P/(R*T)\nP = 101.325e3 Pa\nV = 1 m^3\nR = 8.314472\nT = 273.15 K\n\nN/m^3 = 44.6149 mol/m^3 = 0.0446149 mol/L\n1 mol of F2 = 37.9968 g\n0.0446149*37.9968 = 1.69522 g/L\n\nIf I use 100 KPa (1 bar) as standard pressure, I get 1.67305 g/L\n\nThe difference in the values given in the answer and the "Handbook of Chem. & Physics" is apparently due to the shift from 1 atm to 1 bar as the definition of "standard pressure."\nI think the slight difference in my calculated value and the published one may be due to the fact that when you start getting out to that many decimal places even "ideal gases" aren't totally ideal....maybe I should try the Redlich-Kwong EOS...\n\nOooooops!  I didn't want to do your homework for you...maybe I should erase all this....:)
33182
We'd need a formula editor to do this...\n\nPressure difference delta-p must equal vapour pressure p(x) in order to get the vacuum on top of a manometer.\n\nPressure is force F divided by area a.\n\nF is mass m times gravity acceleration g\n\nmass m is density rho times volume V\n\nThe column inside the manometer exerts a pressure \n\np(i) = g * rho * V / a\n\ng: gravity acceleration\nrho: density\nV: volume V=h*a\na: area\nh: height  h=V/a\n\nso we get\n\np(i) = g * rho * h
35270
G is for guage, which uses ambient pressure as the reference point as opposed to PSIA, where A is Absolute, which uses an absolute vacuum as the reference point.
684353
P1V1T2=P2V2T1 \n\nRemember to express  temperature in Kelvin (with pressure in Pascals and volume in m^3)
966327
I agree; c) is the right choice.  The other units are used to measure:\n\na)  power ratio\nb)  pressure\nd)  pressure (again)
238622
it is the normal force per area...\nyou can visit this site:\nhttp://en.wikipedia.org/wiki/Pressure
665350
As the volume is constant,\n(P/T)initial = (P/T) final\n1/(25+273.15) = P/(50+273.15)\nP = 1.084 atm\n\n(Taking the pressure of the initial gas was 1 atm.
967963
Either air pressure, or fluid pressure on a fluid present in the cylinder.
869862
I dont understand what r u doing with "p*v/t"; but if assume ideal gas behavior, PV = nRT, so P = nRT/V [n is number of moles, R is ideal gas constant, T is temperature, V is volume of the flask, P is the pressure]
360638
I'm thinking that you meant to type pressure instead of height. because millibars do not measure height. they measure pressure. and altitude and height are pretty much the same thing.\n\nthe relationship between altitude and pressure can be modeled by this equation\n\nlog(.01*P)~5-(h/50853.0185)\n\nwhen P=pressure in millibars and h=altitude in feet