Question

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

Answer #1

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.

One mole of ideal gas initially at 300 K is expanded from an
initial pressure of 10 atm to a final pressure of 1 atm. Calculate
ΔU, q, w, ΔH, and the final temperature T2 for this expansion
carried out according to each of the following paths. The heat
capacity of an ideal gas is cV=3R/2.
1. A reversible adiabatic expansion.

One mole of an ideal gas does 3000 J of work on its surroundings
as it expands isothermally to a final pressure of 1.00 atm and
volume of 25.0 L. Determine:
a) the initial volume ?
b) the temperature of the gas?
(Note: 1 atm = 1.01 x 105Pa, universal gas constant R
= 8.31 J/mol K, 1 L = 10-3m3)

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.

Consider an ideal gas of 0.2 mole of argon atoms with an initial
volume of 0.8 liter (8*10-4 m 3 ) and a temperature of 300 K.
a) The gas is thermally isolated and allowed to expand
adiabatically to a final volume of 1 liter (10-3 m^3 ). How does
the entropy of the gas change? Please provide your reasoning.
b) Find the final temperature, ?? , of the gas after its
adiabatic expansion.
c) With the gas at the...

One mole of an ideal gas is expanded isothermally and
irreversibly from an initial volume of 10.0 L to a final volume of
20.0 L at a pressure equal to the final pressure and a temperature
of 500 K. Calculate the value of w. Calculate the values of q.
Calculate the value of ΔS (system). Calculate the values of delta S
(surroundings). Calculate the values of ΔS (total).

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

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...

Consider an ideal gas of 0.2 mole of argon atoms with an initial
volume of 0.8 Liter and a temperature of 300K.
a) The gas is thermally isolated and allowed to expand
adiabatically to a final volume of 1 Liter. Find the final
temperature of the gas after its adiabatic expansion.
b) With the gas at the temperature Tf that you calculated in
(a), it is now brought into contact with a large thermal reservoir
at 300K and equilibriates to...

Suppose 4.00 mol of an ideal gas undergoes a reversible
isothermal expansion from volume V1 to volume V2 = 8V1 at
temperature T = 300 K. Find (a) the work done by the gas and (b)
the entropy change of the gas. (c) If the expansion is reversible
and adiabatic instead of isothermal, what is the entropy change of
the gas?

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