Question

Consider a gas of nitrogen molecules at 20°C with a particle
density of 2.7 ×1019 molecules/cm^{3}. 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?

Answer #1

The average kinetic energy of the molecules in a gas
sample depends only on the temperature, T. However, given the same
kinetic energies, a lighter molecule will move faster than a
heavier molecule, as shown in the equation for rms speed rms
speed=√3RTM where R=8.314 J/(mol⋅K) and M is molar mass in
kilograms per mole. Note that a joule is the same as a
kilogram‑meter squared per second squared (kg·m2/s2). What is the
rms speed of Cl2 molecules at 471...

A container holds 2.7 mol of gas. The total average kinetic
energy of the gas molecules in the container is equal to the
kinetic energy of a 8.5x10-3 kg bullet with a speed of 880 m/s.
What is the Kelvin temperature of the gas?

Compute the root-mean-square speed of a nitrogen molecule at
23.6°C. The molar mass of nitrogen molecules (N2) is 28.0×10-3
kg/mol. At what temperatures will the root-mean-square speed be (b)
1/4 times that value and (c) 4 times that value?

Compute the root-mean-square speed of a nitrogen molecule at
60.1°C. The molar mass of nitrogen molecules (N2) is 28.0×10-3
kg/mol. At what temperatures will the root-mean-square speed be (b)
1/3 times that value and (c) 4 times that value?

1. The average kinetic energy of the molecules in a gas sample
depends only on the temperature, T. But given the same kinetic
energies, a lighter molecule will move faster than a heavier
molecule.
A. What is the rms speed of Cl2 molecules at 505 K?
B. What is the rms speed of He atoms at 505 K?
2. Use the van der Waals equation of state to calculate the
pressure of 3.70 mol of H2O at 473 K in...

Chemistry - Gas Laws:
A 1.00 liter vessel contains 5.00 grams of nitrogen (N2) and
1.50 grams of water at 25°C.
a)Determine the RMS speed of nitrogen molecules and water
molecules in the vapor phase at 25°C.
b)Calculate the average kinetic energyper moleculeof nitrogen
and of water vapor at 25°C.
(Show all work and calculations, include units in
answer. If calculations must be used in several parts, rounding
should be made to 6 decimal points to ensure accuracy. Final
Answers...

1. You have two identical containers, one containing gas A and
the other containing gas B. Both gases are under the same pressure
and are at 5.0 ?C. The molecular masses are mA = 3.29 × 10?27 kg
and mB = 6.12 × 10?26 kg.
(a) (1 point) Which gas has greater translational kinetic energy
per molecule?
(b) (1 point) Which gas has greater rms speed?
(c) (1 point) Assuming you can only change one of the
containers, the temperature...

(a) Compute the root-mean-square speed of a nitrogen molecule at
99.1°C. The molar mass of nitrogen molecules (N2) is 28.0×10-3
kg/mol. At what temperatures will the root-mean-square speed be (b)
1/3 times that value and (c) 2 times that value?

Consider a classroom filled with air. Let’s approximate air as
an ideal gas of N2-molecules (nitrogen) at normal conditions (P = 1
Bar and T = 300 Kelvin). Suppose the room has dimensions of 10 m by
10 m by 10 m (a pretty large auditorium). Let us also assume that
N2 molecule has 5 degrees of freedom (3 translational and 2
rotational). In this problem you will need to provide numeric
answers up to the first significant digit.
2.1...

2. An aluminum scuba tank, which has an internal volume of 11.1
L, is filled with air to a pressure of 3000 psi when at room
temperature (i.e. 20.0 OC). A diver takes the tank into seawater,
where the water temperature is 46 degrees Fahrenheit (i.e. 8.00OC).
To what pressure does the air in the tank drop? (The thermal
coefficient of expansion for aluminum is 24.0x10-6 OC -1 .)
Answer: 2880 psi
Don't need #2, just #3 please.
3. For...

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