relationships of pressure, volume, and temperature?
606777
the actual equation is:  (p + b·n^2/V^2)(V - a·n) = nRT\n\na:- every mol of particles of the gas has a tiny finite volume of a\n\nb:-modification is due to the particles sticking to each other, a phenomenon called cohesion\n\nR- rydberg's constant
683503
In the relationship between pressure, temperature and volume of gases, the pressure and temperature have a direct relationship....if one factor goes up so does the other one.  So, set up what you know as a ratio.\n\npressure/temperature = pressure/temperature\n\n400/80  =   300/x       cross multiply and solve for unknown\n\n24000 = 400x\n\n60 = x
276816
Pressure, Temperature, and Mass.  That's just three basic things to measure.  You measure volume, from volume you get density, which is an intensive property.  Pressure is an intensive property.  Temperature is an intensive property.  Volume and mass isn't because if you partition them, they will not be the same, unlike pressure or temperature (assuming there is no temperature gradient), and density.  From these, you could get stuff like entropy, gibbs free energy, figure out work, thermal conductivity, enthalpy, etc.  You just have to look for the right stuff.
397497
I would use the ideal gas law...more specifically...the combined ideal gas law...\n\nP1*V1/T1 = P2*V2/T2
523715
Higher Velocity will cause lower pressure and larger volume that will decrease its temperature. Volume, temperature and pressure are all physically related in gas.
984213
http://en.wikipedia.org/wiki/Pressure_gradient_force\nhttp://en.wikipedia.org/wiki/Temperature_gradient\nHope this helps, good luck!
180516
Well, P * V = n * R * t\nRight side is equal before and after changin` pressure.\nSo, P1 * V1 = P2 * V2\nP1 = 1.01 kPa ;\nV1 = 458 mL ;\nV2 = 477 mL.\nP2 = (P1 * V1)/V2\nP2 = (1.01 kPa * 458 mL)/477mL\nP2 = 0.97 kPa\n\nP.S. You didn't have to say how much is the temperature, it doesn't mather.
368820
changes in air pressure, and temperature at changing locations
534799
Yes.  \n\nBoyle's Law states that the volume of a fixed amount of gas at constant temperature is inversely proportional to the pressure exerted on the gas.  In other words, as pressure rises volume decreases and as pressure decreases volume increases.
715037
Ok-i'm not quite sure if i did this right--we covered this last year--so you might want to double check with your textbook or teacher, or whatever resource you have...\n\nwhat i would do is find the final temperature:\nFinal Temperature=(V2 * T1) / V1\n\nand then use the delta T, delta v, and P to find delta E.\n\nbut i'm really not that sure.\n\nsorry that i wasnt a better help!
569120
Isobars link locations with constant pressure, isotherms do the same for temperature
918910
See if this helps:\nPV = nRT = NkT, where P is pressure, V is volume, n is the number of moles, N is the total number of molecules, T is temperature, k = 1:38 £ 10¡23 J/K is the Boltzmann constant and R is a universal constant, R = 8:314 J/mol.K.
329557
Try this....\n\nhttp://www.efunda.com/formulae/solid_mechanics/mat_mechanics/pressure_vessel.cfm
818902
You better read something on this:\nhttp://en.wikipedia.org/wiki/Pressure
882010
The volume decrease due to temperature is:\n\n(22+273) / (37+273) = 295 / 310\n\nand the volume increase due to the change in pressure is:\n\n760 mmHg / 675 mmHg\n\n780 mL * (295/310) * (760/675) = 835.7 mL
358671
Gay-Lussac's Law states that for a fixed amount of gas (the number of moles stays constant throughout the problem) and a fixed (constant) volume, pressure and temperature are proportional, the formula is:\n\nP1/T1=P2/T2  \n\nThis means as temperature increases in a fixed volume, the gas exerts more pressure on the container, they expand and hit the container walls and push on them.  If the gas is cooled and kept in the same container, the particles exert less pressure on the container, they're more condensed.\nTemperature must be in Kelvin (K) not Celcius to use the formula.
927436
P1T1/V1 = P2T2/V2\nIn your case there is (apparently) no change in pressure, so the above equation will simplify to:\n\nT1/V1 = T2/V2\n\nV2 = T2V1/T1.\nPlug the numbers you have and find V2.  Remember to convert temperatures to Kelvin.