Why is the statement Boyle's Law(read inside)?
604015
The amount of material and the prevalent temperature haven't changed much, so the pressure and volume are inversely proportional.  As the external pressure on the balloon decreases, the amount of material in the balloon will expand to equalize that pressure.
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.
770990
I don't understand your statement of the problem.  It sounds like it might be an exercise in integral calculus, in which you integrate the expression at hand, evaluate the resulting function at the two limits, and take the difference.
265643
the law state that P(pressure)=K*T(temperature), where K is a constant ,when other things are constant.Any closed vessel which is heated is a real life example of gays rule.But it is important to note that it is imposible to find a completely real example for this rule because it is valid only for ideal gases and for real gases there are some factors which leads to deviations from ideal behaviour
227415
actual pressure of the vapour\ndivided by\nthe maximum pressure of the vapour at 'that' temperature\nequals (in this case) 1 = 100%
980849
The relationship between volume and pressure. Remember that theBoyles' law assumes the temperature to be constant.\n\n  P1V1 = P2V2\n\nV1 = original volume\n\nV2 = new volume\n\nP1 = original pressure\n\nP2 = new pressure
542119
As described by the ideal gass laws, P1 V1 = P2 V2. This means that, as the pressure increases, the voulume of the contained vapor decreases and condences.
304043
Because algebra skills are very lacking in most people. It's just to make sure that they know what the rearranged formula's look like. But you are right, those 2 laws are probably all you need to remember. P=IE is always true, but remember than Ohm's Law is only an approximation for materials that have a linear E vs R graph, such as metals at room temperature. Its not true for semiconductors and gas discharges.
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]
708158
well aside from that you said the vapor pressure is 18.6 and put 18.9 in your calculations, it looks great! Besides, even with that difference, it doesn't change the answer at all, its still .877 atm with both values.
457368
Yes it reads inward/outward.  Why so curious??
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.
838291
Good question!\n\nFirst law of thermodynamics states that the internal energy change ΔE of a system is equal to (Q - W). Where Q is the heat absorbed by the system and W is the work done BY the system on the surroundings.\n\nNow, as you already might be knowing that work can also be expressed in terms of pressure and volume as-\n\nW = PΔV (where P is pressure of the gas inside the system and ΔV is the change of volume)\n\n[Here: "system" = balloon; and "surroundings" = refrigerator]\n\nAnd as the change in volume (ΔV) in the case of balloon stated above is negative i.e it deflates, work must be negative i.e (minus W).\n\nNow, as Q is also negative (heat is given off by the balloon), the equation of First Law of thermodynamics reads-\n\nΔE = -Q - (-W)\nΔE = W - Q\n\nNow, if the balloon was large in volume, the change in internal energy ΔE would be positive and the balloon will either burst or move frantically in the refrigerator shelf.\n\nBut, if the balloon was a small one, it'd slowly become limp and deflate as the Q will overpower W (PΔV) in the equation and the internal energy ΔE will decrease and become negative.\n\nPlease note that I have made a lot of assumptions here that perhaps, might not be so easy to apply practically.\n\nThe points you'd have to consider are:-\n\n1-How tightly the balloon is wound so that air doesn't leak out of it.\n2- Whether or not there's a leakage in the balloon.\n3- The temperature of the balloon.\n4- The material of the balloon.\n\nStrictly speaking, the first law isn't even applicable in this case because the condition in the law is that the system (balloon) shouldn't be allowed to move. Its kinetic and potential energies should both be zero which clearly is not the case with our experiment.\n\nI hope this answer helps!\n\nGood luck!
487526
Sounds like a Math/Science type question to me. Why are you posting it here?\n\nBesides, I have the the slightest idea.
961109
It's good to see people actually thinking about what the terms they're using mean, rather than just plugging them into equations.\n\nBasically, the place where you seem to be confused is here:\n\n"In gas such as water vapour, intermolecular forces of attraction is weak and hence it has low PE"\n\nActually, this means the exact opposite, that the system has very high potential energy. Think about gravity for a minute - if a rock placed at, say, 1 foot above the ground were to fall to Earth, it would not release very much energy. Conversely, if the rock were placed 1 mile above the Earth, it would release a considerable amount of energy. The higher the rock is, the greater it's potential energy. However, the further the rock is away from Earth, the weaker the force of gravity acting on it - thus weak gravitational attraction corresponds to higher potential energy. Similarly with the particles in a gas - if they were to "fall" into a partially bound state such as that of a liquid, they would release energy, and thus the unbound state where the particles are too far away from each other to form bonds is the higher energy state.\n\nThis is not to say that a weaker force always corresponds to a higher energy state - if the reason that the force is weaker is that there is less mass/charge/whatever producing it, that really will lower the potential energy. But in the transition from a liquid to a gas does not change the charge of any of the particles - the reduction in intermolecular forces comes from the fact that the particles are moving out of each other's electrical potential wells, a process which, just like lifting up a rock, raises the potential energy.
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.
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