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I believe the shorter the mean free path, the higher the density. Basically, the closer the molecules are, the more dens it is. That is why when you add pressure, the density goes up ... by this equation.
d = PM/RT
P=pressure
M=molar mass
R=gas constant
T=absolute temperature
Basically, the more pressure put on a gas, the closer it goes to being a liquid... which is denser. The bigger the gas (molar mass) the smaller the mean free path, the denser it is.
However, I do not know how to relate mean free path mathematically to density yet.
Wiki User
∙ 13y ago
Wiki User
∙ 14y agoUnder the same physical conditions (temperature, for example), a dense gas will exert more pressure than one that is less dense. You can picture it this way: If you have a sealed box containing a gas, the pressure of the gas is directly related to the impact of the gas molecules on the sides of the box. If the molecules are heavier, the gas is more dense, and the impacts are more powerful (higher pressure). To get the same effect from a less dense gas, a gas with lighter molecules, you need more frequent impacts, which can be achieved by raising the temperature in the box or by packing in more gas molecules.
Wiki User
∙ 14y agoThe Ideal Gas Law PV=nRT
P=pressure
V=volume
n=moles
R=gas constant
T=temperature
density = grams/volume so Volume=grams/density
substituting grams/density for volume into the Ideal Gas Law
P(grams/density) =nRT
solving for density
P(grams)/nRT=density
grams/mole is molecular weight M so
PM/RT = Density
Wiki User
∙ 12y agothe mean free path in dependent on pressure, since the mean free path equation state that mean free path=k*T/((2)^(1/2))*P*o
so if you double the pressure your actually decreasing the mean free path by half.
Wiki User
∙ 12y agoThe density will increase as pressure increases
Wiki User
∙ 10y agoWhen the gas gets exerted by the pressure the density increases because the gas is getting compressed into a smaller space.
Wiki User
∙ 10y agoNO
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Mean free path of water molecule?
k
What source of weather data would enable a meteorologist to follow a path of an approaching thunderstorm?
Meteorologists depend on the air pressure to forecast an approaching storm
At a constant pressure how does a volume of gas vary with respect to the absolute temperature?
It doesn't. The equation for mean free path is: mfp = 1 / [sqrt(2)*n*pi*d^2] In the above equation, n is the number of molecules per unit volume, and d is what is known as the collision diameter (the distance between the centers of the two colliding molecules). Thus, there are only three variables which affect mean free path: number of molecules, volume, and collision diameter. Volume can be changed by a change in temperature, but this question assumes constant volume (meaning pressure will change as temperature changes). As long as the amount of gas is unchanged, the mean free path will be unaffected by changes in temperature. This is a wrong answer. The collision diameter decreases with the increase of temperature.
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Heat and work are path functions because their values depend on something moving from an initial to a final state.
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path is path it is very free of coast because it is hope this answer will effect you
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mean free path
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k
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What source of weather data would enable a meteorologist to follow a path of an approaching thunderstorm?
Meteorologists depend on the air pressure to forecast an approaching storm
What is difference between path function and point function in thermodyanaMICS?
Path function: Their magnitudes depend on the path followed during a process as well as the end states. Work (W), heat (Q) are path functions.The cyclic integral of a path function is non-zero. work and heat are path functions.Point Function: They depend on the state only, and not on how a system reaches that state. All properties are point functions.The cyclic integral of a point function is zero. properties are point functions, (ie pressure,volume,temperature and entropy).
At a constant pressure how does a volume of gas vary with respect to the absolute temperature?
It doesn't. The equation for mean free path is: mfp = 1 / [sqrt(2)*n*pi*d^2] In the above equation, n is the number of molecules per unit volume, and d is what is known as the collision diameter (the distance between the centers of the two colliding molecules). Thus, there are only three variables which affect mean free path: number of molecules, volume, and collision diameter. Volume can be changed by a change in temperature, but this question assumes constant volume (meaning pressure will change as temperature changes). As long as the amount of gas is unchanged, the mean free path will be unaffected by changes in temperature. This is a wrong answer. The collision diameter decreases with the increase of temperature.
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Displacement and overall distance are but the distance travelled does depend on the path.
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yes
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state function did not depend on the path , it depends on the initial and final point of the system where as path function depends on the path of the reaction.
