How does Raoult's Law work?
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Raoult's Law describes a colligtive property.  It states that the more particles that are in solution, the lower the vapor pressure of the solution is.  For example, if I had a beaker of water out and I poured some salt in, the vapor pressure of the salt water would be lower than pure water's vapor pressure.  \n\nMathematically:\nVapor Pressure of the solution = (mole fraction of the solvent) * (Vapor pressure of the pure solvent)\n\nThe mole fraction of the solvent is found by dividing the number of moles of solvent by the total number of particles in solution.  \n\nRaoult's Law works because as more particles are added to the solvent, those particles that are being added block the vapor of the solvent from rising and escaping.  That means that the more particles added, the more vapor pressure blocking, and the lower the vapor pressure of solution.  \n\nRaoult's Law can also alternately apply to when two volatile substances (two liquids that evaporate readily) are mixed together. All you do to calculate total vapor pressure over the mixture is add the two vapor pressures together for the substances.
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gasoline is obtained from the fractional distillation of crude oil.  It is therefore a hydrocarbon.  It is evaporated and mixed with air and forced into the cylinder where it burns.  When the C--C and C--H bonds are broken, energy is required but then more eneryg (than is required to break these bonds) are given off on the formation of H--OH (water) and O--C--O (carbon dioxide)bonds.  This is the thermal energy that causes the burned gas in the cylinder to expand thus forcing the piston away from the spark-plug end, causing the engine to "run"
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(I just did this today in lab with bacteria instead of onions!) Other liquids can do many things to DNA, but water binds to the DNA and "elutes" it, the DNA will stay with the water. (look up "elute")
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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.
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Good question.  The flame converts wax into chemicals that evaporate into the air. Here's how it works:\n\nThe heat from the flame melts the wax into a liquid.  The liquid is drawn up the wick by a process known as capillary action.  The liquid wax is heated by the flame until it turns into a gas.  The gaseous wax combines with the oxygen in the air.  This chemical reaction produces many chemicals, but since wax is a hydrocarbon, (it contains mostly hydrogen and carbon, just like other flamable chemicals such as gasoline and wood) the byproducts are mostly water (a combination of hydrogen and oxygen) and carbon dioxide (a combination of carbon and oxygen).  In the heat of the flame, both water and carbon dioxide are gasses and float away into the air.  That is where the wax goes when the candle burns.
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Boyles law related the pressure and volume of a gas, as pressure goes up volume goes down and vice-versa. Charles law related temperature and volume, as temp goes up so does volume and vice versa.\n\nThe collapsing can demo really does not show either of these laws. If you boil a small amount of water in a can for a few minutes the water will turn to water vapor and expel most of the air out of the can. Then you need to invert the can and place it in cold water. This will seal the opening AND cause the water vapor in the can to condense. After the vapor condenses to liquid water, it takes up less space--- this decreases pressure inside the can, and higher air pressure outside the can crushes it. Not related to either law because they deal with gasses only, not gasses that change state to a liquid.
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How capillary action makes water go up...???\n\nEven though we usually think of water as running downhill, it can indeed flow upwards using a process called capillary action (pronounced kap uh LAR ee, is the tendency of liquids to move into or out of tiny, hairlike passageways) . This is the very scientific principal that explains how water goes from the soil upwards into the stem of plants. Plants contain many vein like tubes that carry water from the plant's roots upwards to the plant's highest leafs via capillary action. Try this experiment to see capillary action in action.\n\nWrap the plastic wrap around the knitting needle and then tape the edges so that you have formed a tube. Remember, the narrower the tube, the more pronounced the capillary effect will be. \nOnce you have taped the plastic wrap, pull out the knitting needle. Make sure that the new plastic tube is not bent and is open at both ends. \nNow pour a little of the food coloring into a glass half filled with water. \nNow place your plastic tube into the glass of water. \nExamine the tube carefully. The dye should climb up the tube above the level of the liquid in the glass. \nNow try the same experiment with varying levels of water in the glass. Does this make a difference?
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The easiest way to understand osmosis is to think about a bottle of strong perfume.  When you take the lid off the molecules spread out filling the room slowly with smell.  Molecules move from an area of high concentration to an area of low concentration.  (that is your answer, I believe)  Another way to understand it is to drop food coloring into a large bowl of water.  It will slowly spread throughout the bowl.
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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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Since you are referring to the volume of the water container and not the volume of the water itself...then the container should have at least twice the volume of the water, so that if another liquid having the same volume of the water will be added to the water in the same container, no spilling will happen. And there are many other liquids that can be added...\n\nHowever, if you made a mistake and you are referring to the volume of water after all, and the original volume of water will not change even if another liquid with the same volume will be added, then that other liquid can be LPG (liquified petroleum gas?!?). The volume of water will not change since, at ordinary temperature, the LPG when poured(?) to the water container will instantaneously change to gas, and therefore, no liquid will be effectively transferred to the water container. Therefore. no change in volume will take place!
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Basic Mechanics 101:\nThe Carburator mixes gas and air. The valve puts the mixture in the cylinder. The pistons compresses the mixture to a flash point. The spark plug provides a spark. The mixture burns up, pushing the cylinder, that turns the crank shaft, which turns the main shaft that is connected to a transmission or to what ever it is you want to turn.
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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.
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Gases are ultimately soluble in each other as noted by the atmosphere. If the pressure is increased, the molecules will get closer together.  But, the solubility stays the same.
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There are gasses dissolved in the fluid. When you stretch the joint the volume increases and therefore the pressure in that volume decreases. This allows to gas to come out of the liquid. It makes a noise like opening a bottle of soft drink. This is also the same principle that gives divers the bends if they come up too quick. \nThere is a name for the law, it is to do with dissolving gasses in a liquid under pressure. I am suffering a mental block, err henry's law?? russels?? errr.. some plain name like that anyway
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through a process called "Cracking"\nthis is when you take a larger molecule and crack it into smaller more volatile molecules\nthey use this in oil refineries to turn crude oil into more valuable products
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This is really a trick question.  The contents inside a closed (pressurized) can or bottle contains two phases.  The lower phase is a liquid solution and the upper phase is pressurized gas containing a high percentage of carbon dioxide (this is a gas solution).\n\nWhen the container is opened, the pressurized gas excapes into the atmosphere and upon doing so allows a change to take place in the solution below.  The chemical change is:\n\nH2CO3 (aq) --> H2O (l) + CO2 (g)\n\nThe gas bubbles of carbon dioxide form inside the liquid solution, turning it into a mixture (I doubt that the term mechanical has much meaning here).
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Do you know distructive distilation?\n\nIn distructive distilation naturally occuring mixtures like coal, crude patrolum, wood etc. are heated in absence of air. This avoids combustion.\n\nWhile heating the volatile substances immediately vapourize. The remains are further heated and in this way all substances (compounds or elements) gradually are separated from the main body leaving behind the residue. This residue is distillate.