is the pressure of a fixed mass of gas proportional to its volume?
534799
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.
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.
1153522
The quantities you have listed are in fact related via the ideal gas law.  So, assuming you aren't in huge temperature or pressure extremes, you can use the ideal gas law with decent results.\n\nIdeal Gas Law\nPV = nRT\n\nwhere P = pressure (N/m^2)\nV = volume (m^3)\nn = number of moles of gas\nR = universal gas constant = 8.3145 J/(mol*K)\nT = temp (in Kelvins)\n\nSo, by looking at the equation you can not convert air pressure directly to volume without also knowing the temperature and number of moles of gas.
979511
a) If the subject was a gas, you can use Boyle's Law to calculate the change in volume. The Boyle's Law states that the pressure of gas is inversely proportionate to its volume, and hence P1V1 = P2V2.\nHowever, Boyles Law only covers the case of gas, and liquids are only VERY SLIGHTLY compressible. the volume of water doesnt really changes.\n\n***Anyway, how do u even carry a litre of water in an ocean? u can use a bubble, and you cant use any use any hard cased material cos tt will prevent you from finding the change in volume!\n\nb) ???\nUnless you are so sure you can find the change in volume, the density remains the same. I don't know any formula similar to Boyles Law that can explain the relation between the pressure of water and its volume.
280201
Density = mass/volume
1149287
pV = n R T => if pressure is constant => p = n R T / V = const. => p / n R = T/ V = const.\n=> T / V = const.\nT1 = 333 K\nT2 = 533 K\nV1 = 0.2 m3\n\nT1 / V1 = T2 / V2 =>\nV2 = V1 x T2 / V2 = 0.2 x 533 / 333 = 0.32 m^3\nanswer D is correct
930130
I will look at it from a different angle.\nConsider the equation of state,\nPV=MRT\nExpansion through a nozzle causes the\npressure to drop and volume to increase \nbut not as compared to drop in pressre. \nThe net effect is that product PV reduces.\nM the mass is not changing. R is the gas \nconstant. So T[temp in absolute] has to drop.
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
979011
It is also affected by pressure only if one of the constituents is a gas.
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
791045
The volumetric flow rate is proportional to the pressure at the bottom (which is rho*gh, or density times gravity times fluid height) and to the area of the orifice (which is pi*r^2, where r is the radius, 1 mm = 0.001 m).  There is a valve constant involved, which you can assume is equal to 1 if you're not given additional information.
168650
Ideal gas law: PV = nRT.\n\nno change in pressure (P), no change in ideal gas constant (R), no change in number of moles of gas (n). Temperature (T) was multiplied by 1.6, so volume (V) must also. The answer is d.
139840
The formula for either is P=rho*g*h, where rho is the density of the material (mass per unit volume) and g is acceleration of gravity, and h is the depth of the material at which you are measuring the pressure. \n\nPressure is a force per unit area. If force are unbalanced, then one gets acceleration of something i.e., something moves, by Newton's second law, F=ma.
1112212
Boyle's Law states that the product of the volume and pressure of a fixed quantity of an ideal gas is constant, given constant temperature.  Mathematically, PV = K, where K is a constant.  So, if the volume or the pressure is changed, the other changes accrodingly.  For example, let's assume the volume of gas is V1 and the pressure is P1.  If we change the pressure to P2, the volume will change to a new volume (V2) such that P1V1 = P2V2
203787
There are a couple of things you need to think about so you can work this out for yourself. \n\n1. Gases expand when they are heated. This is easily seen from the ideal gas law, PV=nRT, where P is pressure, V is volume, n is number of moles, R is a constant and T is temperature. Most gases roughly follow this law. As T increases, so does V, at constant P (of course, in the case of a balloon, P does not remain constant). \n\n2. When the volume of a gas increases, its density D=mass/V  decreases.\n\n3. By Archimedes principle, the buoyant force on an object is equal to the weight of the fluid displaced. The net buoyant force is the difference between the buoyant force on the object and the weight of the object. \n\nSo in the case of your balloon, if it displaces air of greater density (since it is colder), then there is going to be a net buoyant force upwards on the balloon. The weight of the air of density Da displaced by a balloon of volume V is V*Da*g, where g is the acceleration of gravity. \n\nI could go into more detail, but you might enjoy working this out for yourself. If you need more help, then ask.
485920
Size or Mass is directly proportional to energy or power\nFor example :\nPotential Energy - mgh where m stands for mass\nKinetic Energy - 0.5mv^2 where m stands for mass
22880
There's a formula for volumes of gasses:\n\nPV = nRT.\n\nIf I remember right, P = pressure, V = volume, n = number of moles, T = temperature, and R = molar density, or something molar that is specific to the gas.