What law states a relationship betwween volume and Temperature?
415248
The ideal gas law (not sure if it has another name) establishes the relationship between volume and temperature and other things.  Its form is PV = nRT.  There is also Charle's Law and a few others.  Charle's law shows the direct relationship between temp and volume in V/T = k where k is a constant.  It shows that when T increases V must also increase in order for k to remain constant.
845517
One way is to use the Clausius-Clayperon Equation.  See the link below and use the boiling point of water for one of the pressure and temperature pairs.  \n\nP.S.  It's equation 22 in the linked document.
795464
wow... opposite answers to the same question... hmmm In a sense, they are both correct. The volumetric changes experienced by solids due to temperature changes is very small, but there is a slight change indeed. Every solid has its own coefficient of volumetric change for every degree change in temperature. A prime example of solids changing volume are the expansion joints you see in bridges. Also, I think the empire state building is like 6 inches taller in summer than in winter... something like that. Gasses on the other hand experience much larger volumetric changes. Temperature as well as pressure will greatly affect the volume of a gas. Consider oxygen, it can be compressed to a liquid. \n\nOn the other hand, let me second guess this question, maybe it should read, why can a gas be compressed and not a liquid? In a gas, the molecules are spaced wide apart, farther apart than their electric charges do not affect the molecule next to them. In a liquid, the molecules are packed as tight as they physically can be packed. They cannot be compressed farther. Only temperature can affect the volume of a liquid as mentioned above. Hope this helps some!
1167777
D.  Based on the ideal gas law, PV=nRT\n\nSolve for R to get: R = (P*V)/(n*T)\n\nfor two different conditions, then, you would have:\n\n(P1*V1)/(n1*T1) = R = (P2*V2)/(n2*T2)  or,\n\n(P1*V1)/(n1*T1) = (P2*V2)/(n2*T2)\n\nor P1*V1*n2*T2 = P2*V2*n1*T1\n\nNote how V1 and T1 can never be in the numerator together?  \n\nIn order for the ratio to work, one must be the numerator, the other the denominator, because volume is directly proportional to temperature -- the higher the temperature (keeping number of moles and pressure equal), the larger the volume.
523715
Higher Velocity will cause lower pressure and larger volume that will decrease its temperature. Volume, temperature and pressure are all physically related in gas.
683503
In the relationship between pressure, temperature and volume of gases, the pressure and temperature have a direct relationship....if one factor goes up so does the other one.  So, set up what you know as a ratio.\n\npressure/temperature = pressure/temperature\n\n400/80  =   300/x       cross multiply and solve for unknown\n\n24000 = 400x\n\n60 = x
784131
Charles Law:  Vol and temp are directly proportional; so set up a proportion.  Remember to change temperature to Kelvin by adding 273 to the celcius temp.\n\nV1/T1 = V2/T2 \n\nin your q.1, T2 is your unknown; solve for it.  The answer will be in Kelvin; if you need celcius, subtract 273.\n\nin your q. 2 V2 is your unknown; solve for it.\n\nTo get Charles Law from Ideal Gas Law (PV = nRT) consider the following:\n\nP1V1 = n1RT1:   rearrange the T1 and P1 to get:  V1/T1 = (n1R/P1)\n\nthen\n\nP2V2 = n2RT2;  rearrange the T2 and P2 to get:  V2/T2 = (n2R/P1)\n\nbut in Charles Law n1=n2 and P1 = P2 (number of moles and pressure are consant; R is a constant) so you can write:\n\nV1/T1 = (nR/P) = V2/T2 and so V1/T1 = V2/T2\n\n(if a = b = c, then a=c)
347041
density has to do with the relationship between mass and volume. Water has a density of 1. As long as the mass stays in the same relationship with the volume of water, it has the same density.
827524
Easier compared to one with a higher heat capacity:\n\nH/(m*Cp) = (delta T), where m is the mass of the object, H is the heat that must be added (or removed) to raise (or lower) its temperature, delta T is its change in temperature, and Cp is its heat capacity. From the above formula, you can see that larger values of Cp result in small temp. changes, for the same heat amount.
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.
782736
If ideal gas law is obeyed...\n\ndensity = mass/V == n/V\n\nPV = nRT\nP = (n/V)RT\n\nIf temp is held constant then increasing density increases pressure.
688085
density it mass per volume.\nlitre is a measure of volume.\n\nvalidity is not a physical quantity.
882394
Density=Mass/volume, Therefore heating a gas increases its volume. This change has to be compromised by either mass or density. Mass cannot vary as it's a constant, so the density has to give way. Hence the change in density. When volume increases, density decreases as they are inversely proportional.
856026
Use the gas law\nPV=nRT
33029
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.
94789
Use Boyle's Law for that. Assuming the temperature is always constant, the product of pressure and volume is always constant.\n\nP * V = k\nor\nP1 * V1 = P2 * V2\n\nIf temperature is included in the equation, you could either use the combined gas law or the ideal gas law.\n\nNote: Elevation plays a significant role in Boyle's Law so it will have a difference in the gauge readings if you relocate it from sea level to the mountaintop.
143220
Yes, only if the volume difference is enough to compensate for the difference in temperature.\n\nOtherwise, no.  It is not logically or physically possible, given the same amount and the same environment.