Question

The ideal 1 mol atomic gas with a pressure of P, volume V expands, causing the pressure to be 2P and volume 2V. Find the change in entropy in this process

Answer #1

A mole of a monatomic ideal gas is taken from an initial
pressure p and volume V to a final pressure 3p and volume 3V by two
different processes: (I) It expands isothermally until its volume
is tripled, and then its pressure is increased at constant volume
to the final pressure. (II) It is compressed isothermally until its
pressure is tripled, and then its volume is increased at constant
pressure to the final volume. Show the path of each process...

An
ideal gas expands quasistatically and isothermally from a state
with pressure p and volume V to a state with volume 6.9V. How much
heat is added to the expanding gas? (Use any variable or symbol
stated above as necessary.)

A 2.00-mol sample of a diatomic ideal gas expands slowly and
adiabatically from a pressure of 5.04 atm and a volume of 13.0 L to
a final volume of 31.0 L.
(a) What is the final pressure of the gas?
atm
(b) What are the initial and final temperatures?
initial
K
final
K
(c) Find Q for the gas during this process.
kJ
(d) Find ΔEint for the gas during this
process.
kJ
(e) Find W for the gas during...

An ideal gas is held in a container of volume V at pressure p.
The rms speed of a gas molecule under these conditions is v. If now
the volume is changed to 4V , the rms speed of a molecule will
be

3. 10.0 moles of ideal gas cloud has an initial pressure of 1.00
bar, initial volume of 100.0L and temperature of 25.0ºC. The cloud
expands adiabatically to a final volume of 1000.0L. Cp,m= 20.79 J /
mol K (Cp,m is molar heat capacity and constant pressure)
a. (10 pts) What is the final pressure of the gas cloud?
b. (10 pts) What is the final temperature of the gas cloud?
c. (10 pts) What is the change in entropy for...

One mole of an ideal gas at atmospheric pressure expands
isobarically from a volume of 1m3 to a volume of
2m3.
1 - Find the initial and final temperatures of the gas
2 - Find the work done by the gas
3 - Find the heat added to the gas

1 mole methane gas (NOT ideal gas) isothermally expands from
initial pressure of 5 bar to 1bar at 50oC. Estimate the ENTROPY
change (?S) for the gas using Lee/Kesler generalized correlation
tables

One mole of an ideal gas initially at temperature T0 reversibly
expands from volume V0 to 2V0,
(a) at constant temperature (b) at constant pressure.
Calculate the work, the heat, and change in internal energy of
the gas in each process.

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

Calculate the total change of entropy for an ideal monatomic gas
expanding from a volume V into a volume 2V via: i) Free expansion
ii) Quasi-static isothermal expansion iii) Quasi-static adiabatic
expansion; iv) Do the results of (iii) surprise you? Comment on
what these results mean in terms of reversible and irreversible
processes.

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