Proving Dalton's Law of Partial Pressure?
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?
918434
One of the basic principles of physics (Newton's Third Law) is that for every action (force) there is an opposite and equal reaction (force). The principle of a rocket motor may be understood by considering the example of a closed container filled with a compressed gas. Within this container the gas exerts equal pressure on every point of its walls. If a hole is punched in the bottom of the container, however, the gas at the bottom escapes and the pressure against the top of the container is no longer equalized. The internal gas pressure then pushes the container upwards in reaction to the jet of air escaping downwards. The amount of thrust developed by a rocket motor depends mainly on two factors, the velocity with which the burning gases leave the combustion chamber, and the mass of the burning gases.
482843
Boyle's law\n\nP1xV1=P2xV2\n\n(.75 atm)x(2 L) = (2 atm)x(X)\n\n1.5=2x\n\ndivide both sides by 2\n\n.75 L would be the volume of helium if the container was at a pressure of 2 atm.
843756
USE PRINCIPLE OF CONSERVATION OF linear MOMENTUM.\n\nearth gas lower KE because it has huge mass and huge inertia
494151
It's bernoulli's principle. Fluids have a lower pressure when moving than when still. Since the water is moving past the spoons (which act like the wing of a plane) they feel a pull from the pressure drop and come together. Try it with a peice of paper sometime. Roll a piec of paper up so when you place it on a flat surface it looks like a curved bridge. then blow under it and it will collapse instead of blow away. It's pretty neet.
652894
the amount of pressure exerted on an object
259405
Total volume =( 1 + 2 ) dm3 = 3 dm3.\nUse Boyles  pV = constant on both gasses.\nThe partial pressure of helium is 2/3 kPa.\nThe partial pressure of neon is also 2/3 kPa.\nDalton's law:\nthe pressure of the mix is 2/3 kPa + 2/3 kPa = 1.3 kPa.
1075715
Here are two sites that look into the problem:\n\nhttp://www.kw.igs.net/~jackord/bp/f6.html\nhttp://math.fullerton.edu/mathews/N310/projects/e6.htm
272822
One cool way that I have seen it derived is based on Jayne's Formalism.\n\nAssume we sample process, and measure the mean and standard devation of the samples. There are many possible distributions that will produce those exact mean and standard deviation. \n\nJayne's Formalism chooses the distribution which maximizes the entropy of the distribuiton. This is viewed mathematically as the distribution that makes the minimum number of assumptions regarding the distribution.\n\nI always thought that was kinda cool.
936208
Geez, that's a beast of an assignment if you haven't even heard of these laws before.\n\nNone of these laws are recent, so any good encyclopedia should have lots of information about them.  Even Wikipedia, but always take wikipedia with a grain of salt, since it's nonprofessional and many professors don't accept citations from it.\n\nThe gas laws should be pretty well covered in an elementary chemistry textbook.  I really can't recall if such a book would cover Fickian diffusion, but Dalton's law and Henry's law should be in there as well.  If you have a chapter in your course textbook about blood chemistry, that might be a place to look, as Dalton's law deals with the partial pressure of gases, and Henry's law with the solubility of gases in liquids.  Fick's law would certainly be covered in any references about the lungs.
276235
Unfortunately, this question can not be solved because it lacks pertinent information that is required to solve the problem.  But, I will lead you through the steps as if all the information were present.\n\nThe first step would be to determine how many moles of substance is present, the temperature(in Kelvins), and the volume(in L), using the R value of .0821.  This plugs into the equation PV=nRT.  Solve for P, which gives the total pressure of the system. \n\nThe next step is to determine the mole fraction for each of the substances.  This is accomplished by dividing the number of moles of the particular substance by the total moles used earlier.  This value is the mole fraction.\n\nFrom here, to find the partial pressure for the particular substance, multiply the mole fraction by the total pressure of the system.  This will give you the partial pressure for that substance.\n\nThen, using Dalton's Law of Partial Pressures, subtract the partial pressure value from the total pressure to determine the partial pressure of the other substance.  Now, the problem is solved.  Thus, the substance with the greatest mole fraction will have the greatest partial pressure.
497010
DUE TO SURFACE TENSION POSITIVE ANGLE OF CONTACT AND INTERNAL PRESSURE.
569322
Use the ideal gas law \n\nPV/T = constant for the final and initial states.
203626
it is RAYLEIGHS THEORY
870041
This question does indeed deal with Dalton's law with the stipulation that the total pressure of the "wet gas" is referring to the oxygen collected in gas form combined with the water vapor collected from water evaporation.  Therefore, all you need to do is figure out what the pressure of water vapor is at 20 degrees Celsius.  Convert to mm Hg if you need to and there you have it.  Subtract the two and what's left is the contribution of the oxygen.  \n\n760 mm Hg = 101.325 kPA just for quick reference.  Hope this helps!
193517
You don't provide enough data to determine this.  The gas law PV=nRT has variables you need to define.
119796
This is true iff the pressure P1 = P2 = const.