Question

Find the mean free path of nitrogen gas at pressure p = 2.5atm and temperature T = 56.50F. The diameter of a nitrogen molecule is d = 0.3 nm. What is the average rate of collisions?

Answer #1

7. A nitrogen molecule has a diameter of about 0.29 nm. The mean
free path of a nitrogen molecule in a tank of dry nitrogen at room
temperature (293 K) and standard pressure (1 atm) is about 0.10 µm.
A tank containing nitrogen at standard temperature (273 K) and
pressure has volume V. If the tank is compressed by means of a
piston to 20% of its original volume, what is the mean free path
for a nitrogen molecule under...

The mean radius of a molecule of a certain gas is R=0.1 nm , and
the molar mass is 18 gram/mole. If pressure P=1.01x105
Pa and temperature T=300K
a) What is the mean free path , λ?
b) If a molecule of the gas has diffused a distance of 12m, what
is the number of collisions this molecule has undergone?

3. Derive the mean free time and mean free path of a gas
molecule. Calculate both these parameters for a nitrogen molecule
at T = 27 degree Celsius'
*Please show formulas, steps, descriptions.

A cylinder of nitrogen gas has a volume of 1.3×104 cm3 and a
pressure of 90 atm What is the thermal energy of this gas at room
temperature (20∘C)? What is the mean free path in the gas?

1. Estimate the following for a nitrogen molecule. The diameter
of a nitrogen molecule is approximately 0.300 nm.
Estimate the mean free path of a nitrogenmolecule in air at the
top of Mt. Everest (altitude = 8.80 km, P ≈ 50.0 kPa, and
T ≈ 238 K). Value of Boltzmann's constant is
1.381×10−23 J/K (answer is in nm)
3. A tank of compressed air of volume 1.00 m3 is
pressurized to 27.0 atm at T = 273 K. A valve...

The mean free path is the average distance travelled by a
molecule, atom, particle, etc. between a collision with another
particle or molecule. Calculate the mean free path, ?, of air at
room temperature, T = 71.2

Calculate the pressures, P, in atmospheres at which the mean
free path, l, of a hydrogen molecule will be 3.50 μm, 3.50 mm, and
3.50 m at 20.0 °C. The diameter of a H2 molecule is 270 pm.

The pressure exerted by a molecular hydrogen gas at a
temperature of 7oC is 1.01x105 Nm-2. Assuming the hydrogen
molecular diameter is 2.0x10-10 m, and the mean speed is 860 ms-1,
evaluate:
(a) the mean free path, [6]
(b) the mean time between collision and [3]
(c) the collision frequency [3]
Useful constant: kB = 1.38 x 10-23

Consider a gas of nitrogen molecules at 20°C with a particle
density of 2.7 ×1019 molecules/cm3. The molar mass of
nitrogen molecules is 28 g/mol.(a) What is the rms speed of the
nitrogen molecules?(b) At what temperature will the rms speed be
half that value?(c) What is the average translational kinetic
energy of these molecules at 20°C? (d) The mean free path of the
nitrogen molecules is 0.80×10−5 cm. What is the molecular radius of
a nitrogen molecule?

A cylinder of nitrogen gas has a volume of 1.3×104 cm3 and a
pressure of 90 atm .
part A: What is the thermal energy of this gas at room
temperature (20∘C)?
Express your answer to two significant figures and include the
appropriate units.
Part B. What is the mean free path in the gas?
Express your answer to two significant figures and include the
appropriate units.

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