An explanation of raoult's and henry's law?
481349
Ana nailed it for you, but see the molecular discussion and math of the link.
33029
Some of the basis laws that govern the behavior of gases follow:\n\nBoyle's Law= Volume is proportional to the inverse of pressure\n\nCharles' Law= Volume is proportional to temperature\n\nAvaogadro's Law= Volume is proportional to number of moles present\n\nThese together lead to the ideal gas equation:\n\nPV = nRT\n\nwhere P is pressure\n      V is volume\n      n is the number of moles present\n      R is the gas constant\n      T is the temperature\n\nThe value of R is 0.082057 L*atm/(mol*K).\nTemperature must be in kelvins for this relationship.  Temperature in kelvins = tempature in Celcius +273.15.
722185
From this patent\n\nwww.freepatentsonline.com/6962719.html\n\n\n\nThe total extract described in EXAMPLE 1 was loaded in a dialysis bag with molecular weight cut off 500 (Spectra/Por®, Cat. No. 131 057). Both ends of the bag were sealed with clamps. The bag was placed in a bucket contained deionized water, in which the ratio of the supernatant and deionized water was 1:10. The total extract was dialyzed at 4° C. with stirring thrice each for 20 hours. The solution remaining in dialysis bag was collected and concentrated under reduced pressure to give the extract.
155067
The liquid molecules begin to heat up which causes them to increase their moleculer movement. They eventually move very far apart which causes them to be in the "gas" state.
382823
Boyle's law: P1V1 = P2V2. As gases get compressed their volume shrinks. As gases decompress their volume expands. Taking a 1 cubic foot balloon down in the ocean would cause it to shrink to 1/2 its size at 33'. Breathing at depth, ascending, and holding your breath may cause serious lung over-expansion resulting in arterial gas embolism, etc. \n\n\nHenry's law: A gas over a liquid will flow into the liquid until the pressure is equal. If you covered a lake with neon, the atoms of that gas would pass though the surface of the water until the neon in the water had the same pressure as what is left in the air. \n\n\nCharles's law - When you heat a gas in a container that is closed the pressure of the gas will rise. Likewise, if you cool the gas the pressure will drop. Likewise, if you decrease the pressure on a gas it will cool. If you take your scuba tank to have it filled and they fill it fast, the temperature will rise. As time goes by the air and tank will cool down. When that happens the pressure in the tank will drop. So, pressure, temperature, and  changing gas volume are all related. \n\n\nDalton's law: When you have a mixture of gases, each gas contributes to the total pressure. If you have a container of air that is at 2 atmospheres, 21% of the 2 atmospheres (0.42 atm.) is due to the oxygen, and 78% (1.56 atm) is due to the nitrogen. Both gases exert their own pressure and the two are combined to find the total pressure. \n\nThe gas laws are a set of laws that describe the relationship between thermodynamic temperature (T), pressure (P) and volume (V) of gases. Three of these laws, Boyle's law, Charles's law, and Gay-Lussac's law, may be combined to form the combined gas law\n\nP1V1/T1 = P2V2/2\n \nwhich with the addition of Avogadro's law later gave way to the ideal gas law. Other important gas laws include Dalton's law of partial pressures. The kinetic theory of gases, Graham's law of effusion and root mean square velocity all explain how individual molecules in a gas act and their relation to pressure, volume, and temperature.\n\nA gas that obeys these gas laws exactly is known as an ideal gas (or perfect gas). An ideal gas does not exist; however, some gases follow the laws more closely than others given standard conditions.\n\nThe most important gas law is the ideal gas law, which states that:\n\nPV = nRT \n \nwhere\n\nP is the pressure in Pascal \nV is the volume in Cubic meters \nn is the number of moles of gas \nR is the ideal gas constant (8.31 J/mol K) \nT is the temperature in kelvins. \nOther gas laws, such as van der Waals equation, seek to correct the ideal gas laws to reflect the behaviour of actual gases. The van der Waals equation alters the ideal gas law to reflect how actual gases function using a series of calculated values called van der Waals constants.\n\nIt is also possible to apply Boltzmann's analysis to determine further information about gases.
481468
Boyle's law states that the volume of a fixed mass of gas varies inversely with the pressure at constant temperature.\n\nUsing P1 and V1 to stand for initial conditions and P2 and V2 to stand for new conditions results in the following equation.\n\nP1xV1=P2xV2\n\nSimple proportion...\n\nNow, the law relating to pressure and temperature would be Gay-Lussac's law which states the pressure of a fixed mass of gas at constant volume varies directly with the Kelvin temperature.\n\nFor a given mass of gas at constant volume, the ratio P/T is the same for any set of pressure-temperature values.\n\nThe proportion for Guy-Lussac's law would be:\n\nP1/T1=P2/T2\n\nSo, to answer your question, for Guy-Lussac's law, not Boyle's law, a reduction of pressure WOULD cause a reduction in temperature.
211996
Well, I'll start you off.\n\nAbsorbances are additive, so you subtract the blank from the measurement (.214 - .009 = .205)\n\nSo the absorbance is .205. Now you use beer's law, which is:\n\nA = ebc\n\ne is molar absorptivity (in L/mol cm)\nb is path length (cm)\nc is concentration. \n\nYou use that equation to figure out the concentration of the complex.\n\nFrom there, you can figure out the concentration of iodine based on the amount of starch used. Unfortunately, you've not provided enough information to go beyond here.
810276
Well, probably easier to explain empirically -- I know that one of the equations that you would be looking for is Planck's law of black-body radiation.  That, along with other equations involved in transport phenomena could be used to model the system and let you know how much heat you lose from the glass.\n\nOff the top of my head, I can't remember every equation that one would want to use.  Good luck!\n\nThe link is to Wiki's entry for Transport Phenomena -- the first reference there would be an excellent -- if very heavy on the math -- reference for solving this problem.
930130
I will look at it from a different angle.\nConsider the equation of state,\nPV=MRT\nExpansion through a nozzle causes the\npressure to drop and volume to increase \nbut not as compared to drop in pressre. \nThe net effect is that product PV reduces.\nM the mass is not changing. R is the gas \nconstant. So T[temp in absolute] has to drop.
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]
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.
1078399
i'm not very sure if this is what you're looking for, but for a closed system with constant temperature, pV=p'V'. since volume, V = pi x (diameter/2)^2 x length, with constant length of the pipe, we have V = k(diameter)^2, where k is constant. hence, pV=p'V' is rewritten as p(diameter)^2 = p'(diameter')^2, i.e. p'/p =(80/250)^2. the new pressure is 0.1024 the original pressure.
966324
Ether has a higher saturated vapor pressure than water. Thus the former boils at a lower temperature than the latter.
700450
Letters A, B, D.\nIn not sure about C, its wording is tricky.\nIdeal gas law : PV = nRT\nReal gas law : (P + (a(n / V)^2)) * (v - nb) = nRT\nThe corrected pressure times the corrected volume.
558434
dont use PV=nRT... you dont need it for these problems... just requires more work because you have to figure out more than one variable\n\nfor everything here it seems you need different laws\n\nBoyles Law is P1V1=P2V2\nCharles Law is V1/T1=V2/T2\nGuy Lussac's Law is P1/T1=P2/T2\n\nall of those laws are just proportions.. just substitute in the numbers you need.  for temperature problems you need to convert them to kelvin... just add 273 to the celcius temperature and you have the temperature in kelvin.\n\nfor example, look at number one...just plug in all the numbers\n\nsince you're dealing with volume and pressure, you'd use Boyle's Law.\n\nP1V1=P2V2\n\n(3atm) * (15mL) = (2.5atm) * (x)\n\nsolve for x\n\n3 times 15 is 45...  2.5 times x is 2.5x\n\n45=2.5x\n\ndivide both sides by 2.5\n\n45/2.5 = 18\n\nthe volume will increase because there is less pressure.  the volume would increase by 3 mL.\n\nlook for what you are given, find out which law you need, and just plug in the numbers\n\nfor number 4.... since you're dealing with pressure and volume again you'd use Boyle's Law.  Given pressure is STP\n\n(15L) * (1atm) = (x) * (3atm)\n\nsolve for x...\n\n15 times 1 is 15... x times 3 is 3x\n\n15=3x\n\ndivide by 3 on both sides...\n\nx=5L of methane gas.\n\nfor number 5 you're dealing with volume and temperature.  with that we would have to use Charle's law.\n\ncharle's law = V1/T1=V2/T2\n\nnow plug in the numbers...\n\n(450L)/(30+273K)= (x)/(90+273K)\n\n(450L)/(303K) = (x)/(363K)\n\n1.485 = x/363\n\nmultiply 363 on both sides\n\n539.01 = x\n\nthe volume of ethane would be 539.01 L\n\ngood luck
284573
good link below\n\nhttp://en.wikipedia.org/wiki/Kinetic_theory
502267
Transpiration and concentration gradients