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.
Under 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.
The 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
the 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.
The density will increase as pressure increases
When the gas gets exerted by the pressure the density increases because the gas is getting compressed into a smaller space.
NO
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Meteorologists depend on the air pressure to forecast an approaching storm
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.
No, entropy is a state function.
Heat and work are path functions because their values depend on something moving from an initial to a final state.
path is path it is very free of coast because it is hope this answer will effect you
mean free path
k
Density: As gas density increases, the molecules become closer to each other. Therefore, they are more likely to run into each other, so the mean free path decreases.Increasing the number of molecules or decreasing the volume will cause density to increase. This will decrease the mean free path.Radius of molecule: Increasing the radius of the molecules will decrease the space between them, causing them to run into each other more. Therefore, mean free path decrease.Pressure, Temperature, and other factors that affect density can indirectly affect mean free path.
Meteorologists depend on the air pressure to forecast an approaching storm
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).
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.
Displacement and overall distance are but the distance travelled does depend on the path.
the enthalpy of a reaction does not depend on the path
No, entropy is a state function.
yes
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.