Question

Here we calculate the partition function, molar translational internal energy, and molar translational entropy of a monatomic gas. The single particle translational partition function is qtrans=VΛ3) where Λ is the thermal wavelength and teh entropy is given by the Sackur-Tetrode equation S=N*kB*ln((qtrans*e^5/2)/N).

A. Calculate the single particle translational partition function q for neon gas at T=298K and V=22.4L. Assume neon behaves ideally.

B. Based on your answer in Part A, calculate the molar translational internal energy of neon at at T=298K.

C. Using your answer in part A, calculate the molar translational entropy for neon.

D. Calculate the molar translational entropy change ΔS if the temperature of one mole of neon gas is increased to 500K and the volume is doubled from the value in part A..

E. The molar entropy change of an ideal monatomic gas
was given when the temperature changes from T_{1} to
T_{2} and the volume changes from V_{1} to
V_{2.}. Using this equation in terms of the inital and
final tempertures, the initial and final volumes, and R, calculate
the molar entropy change when the temperature of an ideal monatomic
gas changes from T=298K to T=500K and the volume doubles.

Answer #1

These are four options -

Calculate partition function, free energy, thermal energy,
entropy, and pressure of monoatomic ideal gas (only translational
motion is present).

The partition function for a two-dimensional monatomic gas
is
?=?2?????/ℎ^2. Find the internal energy for this two-dimensional
system.

Three moles of an ideal monatomic gas expand at a constant
pressure of 2.90atm : the volume of the gas changes from
3.30*10^-2m^3 to 4.50*10^-2m^3.
Part A, Calculate the initial temperature of the gas.
Part B, Calculate the final temperature of the gas.
Part C, Calculate the amount of work the gas does in
expanding.
Part D, Calculate the amount of heat added to the gas.
Part E, Calculate the change in internal energy of the gas.

17) Three moles of an ideal monatomic gas expand at a constant
pressure of 2.70 atm ; the volume of the gas changes from 3.10×10−2
m3 to 4.60×10−2 m3 .
Part A
Calculate the initial temperature of the gas.
Part B
Calculate the final temperature of the gas.
Part C
Calculate the amount of work the gas does in expanding.
Part D
Calculate the amount of heat added to the gas.
Part E
Calculate the change in internal energy of...

Neon gas (a monatomic gas) and hydrogen gas (a diatomic gas) are
both held at constant volume in separate containers. Each container
contains the same number of moles n of each gas. You find
that it takes an input of 300 J of heat to increase the temperature
of the hydrogen by 2.50°C.
Part A
How many modes does a single hydrogen gas molecule have? (Assume
the vibrational modes are "frozen out").
3, all rotational kinetic
6, 3 translational kinetic...

1. A flask holds 9.73 kg of a monatomic ideal gas (mass number
86.4). If the gas changes temperature isochorically (constant
volume) from temperature 802o C to 376o C,
find the change in the internal energy of the gas, in kJ. A
positive answer means the internal energy increased; a negative
answer means the internal energy decreased.
2. A flask holds 2.25 kg of a diatomic ideal gas (mass number of
the gas 92.1). If the gas changes temperature isochorically...

A tank contains one kilomole of a monatomic ideal gas, argon,
and has a pressure of 1 atm and a temperature of 300 K. The mass of
an argon atom is 6.63 x 10-26 kg.
a.) Calculate the internal energy, U, of the gas in Joules.
b.) Calculate the average energy per atom in eV. (1eV = 1.602 x
10-19 J)
c.) Calculate the partition function, Z.
d.) Calculate the entropy of the assembly, S

Calculate the temperature ? of a sample of gas when the average
translational kinetic energy of a molecule in the sample is
8.15×10−21 J.
?= ________K
What is the total translational kinetic energy ?trans of all the
molecules of this sample when it contains 2.15 moles of gas?
?trans= ________J
A cylinder which is in a horizontal position contains an unknown
noble gas at 54700 Pa and is sealed with a massless piston. The
piston is slowly, isobarically moved inward...

Assume that one mole of a monatomic (CV,m = 2.5R) ideal gas
undergoes a reversible isobaric expansion at 1 bar and the volume
increases from 0.5 L to 1 L. (a) Find the heat per mole, the work
per mole done, and the change in the molar internal energy, ΔUm,
the molar enthalpy, ΔHm, for this process. b) What are the entropy
changes ΔSm of the system and of the surroundings? Is this process
spontaneous? Justify your answer.

Calculate the change in entropy for one mole of ideal gas which
expands from an initial volume of 2 L and initial temperature of
500 K to a final volume of 6 L under the following conditions.
P(initial) refers to the pressure when T(initial)= 500K,
V(initial)= 2 L.
a) Irreversible expansion against a constant pressure of
Pinitial/2
b) Irreversible expansion against a vacuum...a 'free
expansion'.
c) Adiabatic irreversible expansion against a constant pressure
of Pfinal
d) Adiabatic reversible expansion

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