boil's gas law is a reduction in pressure causes a reduction in temperature?
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.
447649
While what everyone is saying is true, if you completely seal the pot the vapor pressure will continually increase and slow or even stop the boiling process (it will make the boiling point significantly higher.)  Actually, if you have an almost full pot in a hermetically sealed container you won't get a boil at all without some seriously massive temps.
72077
Charles' law: If the volume of a container increases, the temperature of the gas inside increases.  If the volume of a container decreases, the temperature of the gas inside decreases.  \nIf the volume of the container increases, then the gas molecules must move faster and impact the walls of the container more often.  Therefore, the temperature must increase as well.
979481
In science you must have studied that the boiling point of water drops with a reduction of atmospheric pressure.\nAt  a pressure of zero atm(atmosphere), which is vaccum, water will boil at room temperature.\nThis boiling is actually the release of the air mixed in the water.\nWhen a pump has a suction  more than 1 atm. which is roughly 27.7 feet, the vaccum created by the pump causes the air in the water to be released as mentioned above.\nThis release of air is known as cavitation.\nCavitation also occurs when the propellor of a boat or ship moves too fast though the water creating a vaccum on the blade surfaces.\nThat is why you see a 'wake' behind a boat or ship
89345
PV=nRT. Standard equation of thermodynamics\n\nPressure * Volumn = constat * Temperator.\n\nA dessicant will remove water from the air, therefore decreases Pressure.  In order for the equation to balance, Temperature will decrease.
82527
This is not chemistry, but physics. I presume you are boiling water in a can, then sealing it and cooling it. There is then less pressure inside the can, since the water takes up less space than the water vapor. There is now more pressure outside the can than inside the can. You have unbalanced forces, and the can is unable to resist the pressure.\n\nThis can of course get far more complicated, and we can discuss the ductility of the can, and continuum mechanics of the can, and its chemistry, but I do not think you want anything that advanced. If you do, let me know.
157020
It is Boyle's law & Charle's Law combined\nVolume of a gas is inversly propotional to Temprature & Pressure.\nOn Cooling can the Pressure & volume is decreased on can\nSince the outer layer of can feels pressure of air & it is more than inner pressure of can So it is crushed
168436
Water boils at 212 F.  The hotter the water, the less energy is needed to achieve this temp.  Of course pressure counts too.  Higher altitudes require different amounts of energy.  I think this is Doyles law.  Chem 101 would be a good class to learn this type of thing.  Also the purity of the water makes a difference.  The less pure the water (minreals, other impurities with lessen the amount of energy needed to achieve boiling temp.
712158
questioner didnt say the gas becomes ideal when volume is increased. he said it MORE CLOSELY approximates.\n\nthis is due to a pressure decrease at constant temperature. (boyle's law). less pressure, atoms further apart, less intermolecular attractions.\n\ncomplete absence of intermolecular forces is a required term in ideal gas principle. so reducing the force obviously creates a more ideal gas.
4765
Boiling is very rapid evaporation starting at the bottom of a container of water.\n\nEvaporation occurs fastest where there is the most heat (energy).  When we heat water to make it boil we heat it from the bottom so the evaporation occurs at the bottom of the pot.  As a result, large  bubbles of water vapor form at the bottom and rise to the surface in the boiling action.  If we applied the same heat to the top surface of the water it would evaporate just as quickly but we would not call it boiling because the bubbles would not form and rise to the surface.\n\nNormally evaporation occurs at a much slower rate than boiling because most evaporation occurs with room temperature water.\n\nEvaporation-is the escape of molecules from the liquid state to the gas or vapor state. In evaporation, molecules of higher-than-average kinetic energy escape from a liquid, leaving it cooler than it was before they escaped.\n\nBoiling-is the temperature at which the vapor pressure of a liquid is equal to the \nexternal pressure above the liquid.  When we give the boiling point of a liquid, we \nneed also to state the pressure.
79685
No.  There was a time when people said it did because some dude in Africa was making ice cream and claimed that his ice cream froze faster if he heated it first, but that's because ice cream needs to congeal, and heating it boiled off much of the water, making it thicker to begin with.\n\nAnd it has been shown even since the time of the Greeks that water that has been boiled prior to freezing will freeze quicker due to the fact that boiling will remove dissolved gases from the liquid, but even that assumes you are comparing water that's been boiled and brought down to temperature versus water that has not been boiled.\n\nBut if you put water that's 8 degrees and water thats 80 degrees in a freezer, the 80 degree water, prior to freezing, will need to reach 8 degrees somewhere between here and there.  All the while, the 8 degree water has made substantial progress towards freezing.\n\nIt is true that hot water loses heat more quickly due to an increased driving force for heat loss, but this is a temporary thing.  As soon as the hotter water reaching the starting temperature of the cooler water, it has no "momentum" in losing heat, but it has lost a lot of time.
931739
By lowering temperature.
947849
The higher the altitude, the lower the atmospheric pressure. The less atmospheric pressure that bears down on the surface of the liquid, the easier it is for water molecules to escape into the air. Thus, the water comes to its full rapid boil at a lower temperature in the mile-high city of Denver than it can in coastal Miami. For each thousand feet above sea level, the boiling point of water drops almost 2° F.
362437
law of conservation of energy\nany gas that is compressed will 'lose' its heat energy to the ambient temperature in the process (ie a refrigerator). in the specific example the gas (1 cm3 at 70F )is at room temperature until its expanded to lets say 1000 cm3, now 70F is spread out 1000x the area,(as is the gas in the can) the more the 70F is expanded the 'colder' it gets (much like the universe or a car tire, but its all relative)
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.
849983
low pressure = lower boiling point = lower dew point
566279
The answer to your question comes from the Charle's law P/T=constant. Thus if pressure decreases temperature will also decrease. Now, the gas in the propane cylinder is not actually cold. When you use the gas, the gas escaping reduces in pressure. So it becomes colder, thus cooling the cylinder.\n\nThis law is true for all gases. So the same will happen with oxygen.