what is sutton's law?
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Sutton's law states that in attempting to diagnose a problem, one should first do the experiment that can confirm the most likely diagnosis. It is taught in medical schools to guide new doctors in ordering tests in a way that leads to faster treatment, while minimizing unnecessary costs. It is also applicable to other disciplines, such as debugging computer programs.\n\nA more through analysis will consider the false positive rate of the test and the possibility that a less likely diagnosis might have more serious consequences.\n\nThe law is named after the bank robber Willie Sutton, who supposedly answered a reporter inquiring why he robbed banks by saying "because that's where the money is." (He later denied saying it.)
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here, you just use the ideal gas law, PV=nRT.  since molarity is equal to moles of solute per liters of solution, M=n/V, so P=MRT.\ntherefore,\nKp=Pco*Ph2o/(Ph2*Pco2)\n  =[CO]RT*[H2O]RT/ ([H2]RT*[CO2]RT)\nall the RT coefficients end up canceling out, so:\nKp=[CO][H2O]/[H2][CO2]\n  =Kc\nsince there were equal numbers of gas molecules on each side of the equation, Kp was equal to Kc.  as a general rule, Kp=Kc*(RT)^N, where N is the change in the number of gas molecules.
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This link should provide the answer and details you may be looking for:\n\nhttp://sulcus.berkeley.edu/mcb/165_001/papers/manuscripts/_971.html
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This could very well be an application of chaos theory (the predictability of random events).  Although as the cables generally find themselves getting messed up, I think this is better described as an application of Murphy's Law.\n\nMurphy's Law, stated mathematically, is "1 plus 1 hardly ever equals 2", or in simpler terms, "If anything can screw up, it will screw up".  This law affects everything from household cables to the antennae of interplanetary probes (as the Galileo team found out when the probe's hi-gain antenna refused to deploy after launch, despite careful design and planning).
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http://en.wikipedia.org/wiki/Law_of_conservation_of_mass\n\nYou're welcome. :]
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You are correct, there is no such thing as "The Law of Probability". However, you could, if pressed by someone, quote it as "Nothing is Always and Everything is Sometimes".
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It varies and isn't really predictable like the Moore's Law.\nhttp://www.ask.com/web?q=moore's%20law
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2nd Law: The Law of Areas, A line that connects a planet to the sun sweeps out equal areas in equal times. This is an empirical law discovered by Kepler, and it has to do with the conservation of angular momentum. When the planet is closer to the sun, it moves faster, sweeping through a longer path in a given time.\n\n3rd Law: The Law of Periods, The square of the period of any planet is proportional to the cube of the semimajor axis of its orbit. This law is a consequence of the law of gravitation by Newton. \n\nSee the examples in the link below:\nhttp://hyperphysics.phy-astr.gsu.edu/hbase/kepler.html
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Cramer's rule is a theorem in linear algebra, which gives the solution of a system of linear equations in terms of determinants. It is named after Gabriel Cramer (1704 - 1752).\n\nComputationally, it is generally inefficient and thus not used in practical applications which may involve many equations. However, it is of theoretical importance in that it gives an explicit expression for the solution of the system.\n\n\nElementary formulation\nThe system of equations is represented in matrix multiplication form as:\n\n \nwhere the square matrix A is invertible and the vector x is the column vector of the variables\n\nhttp://www.answers.com/topic/cramer-s-rule?method=22
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I am not sure what you mean by "General Gas Laws."  The only law dealt with in physics is the Ideal Gas Law which says that pressure and volume are related to amount of gas, temperature and some constant.\n\nPV = nRT
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A blue law, in the United States and Canada, is a type of law restricting certain activities, particularly shopping hours, on Sunday.
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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.
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Coulombs law.\nWhen the distance is made 3 times longer (for instance),\nthe force between the charges becomes 3^2=9 times smaller.
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In physics and mathematical analysis, Gauss's law gives the relation between the electric flux flowing out a closed surface and the electric charge enclosed in the surface.
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The important laws of friction also known as Coulomb's laws of friction are:\n\n1. The frictional force is directly proportional to the normal force between the surface at which it acts.\n(Force required for pulling a block, initially at rest, over a surface is double of that required for pulling another block, of mass twice as the former and initially at rest, over the same surface is double.)\n\n2. Frictional force always acts in a direction opposite to the direction of motion or tendency of motion.\n(If a body is moving relative to another body in contact, then the frictional force acts on both the bodies. It acts on each body in the direction opposite to that of its motion. As the two bodies are in relative motion so the direction of motion of the first with respect to the second and that of the second with respect to the first are always opposite. So the frictional force acts on the two bodies in opposite directions.)\n\n3. The frictional force on a surface is always perpendicular to the normal force. \n(A box can be held over a vertical wall by exerting a force in a direction perpendicular to the wall because the frictional force, perpendicular to normal force, acts in the vertically upward direction thus resisting the downward motion of the box.)\n\n4. Fluid friction is less than solid friction. \n(So liquid lubrication is done in bearings to minimize friction and hence to reduce wear.)\n\n5. In solid friction, rolling friction is less than sliding friction. \n(So it is dificult to pull a cycle with brakes on than without it as when the brakes are on the type of relative motion between the wheel and the road is of sliding type.)\n\n6. The magnitude of frictional force is independant of the area of contact between the surfaces in relative motion. \n(The force required to move two blocks, initially at rest, of different shapes and sizes but with same mass over a particular surface is same. But  for two blocks, initially at rest, with different masses but same area of contact with the surface on which they move the force required to move the one with greater mass is more.)\n\n7. Coefficient of solid friction is independent of temperature.\n(The force required to pull a block resting on a surface does not change with temperature.)\n\n8. Static friction is always greater than kinetic friction.\n(The force required to move a body, initially at rest, over a surface is more than that to keep the same body, initially in motion over the same surface, in moving condition.)
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DeMorgan's Law states that:\nc(A)∩c(B)=c(A∪B) and c(A)∪c(B)=c(A∩B)  (c(x) means the complement set of X)\n\nSupposing that the universal set is {a, b, c, d, e, f, g, h, i},\nc(A)∩c(B) = {b, i},\nc(A∪B)    = {b, i},\nc(A)∪c(B) = {a, b, d, e, f, h, i}, and\nc(A∩B)    = {a, b, d, e, f, h, i},\nso the law is verified. Note that this does not prove the law.
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The same place yo can find many other answers to your questions - Wikipedia.\n\nhttp://en.wikipedia.org/wiki/Hooke%27s_law