Question

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).

Answer #1

For isothermal process,

The equation to calculate work done is given by

, here

Here , , ,

and ,

workdone is considered as negative because the gas expands and the system looses internal energy, or the work is done by the system.

According to first law of thermodynamics,

Since internal energy of the system we get

So

Or

Its assumed that the value of pressure

For isothermal process,

The equation to calculate work done is given by

, here

Here , , ,

and ,

workdone is considered as negative because the gas expands and the system looses internal energy, or the work is done by the system.

According to first law of thermodynamics,

Since internal energy of the system we get

So

Or

Its assumed that the value of pressure

1 mole of ideal gas at 270C is expanded isothermally from an
initial pressure of 3 atm to afinal pressure of 1 atm in two ways:
(a) reversibly and (b) against a constant external pressure of 1
atm. Calculate q, w, ΔU, ΔH and ΔS for each path.

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 expands reversibly and isothermally
from 10. bar to 1.0 bar at 298.15K.
(i)Calculate the values of w, q, ∆U and ∆H?
(ii)Calculate w if the gas were to have expanded to the same
final state against a constant pressure of 1 bar.

1.3 mole of an ideal gas at 300 K is expanded isothermally and
reversibly from a volume V to volume 4V. What is
the change in entropy of the gas, in
J/K?

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 is compressed at a constant temperature
of 55 oC from 16.5 L to 12.8 L using a constant external
pressure of 1.6 atm. Calculate w, q, ΔH and ΔS for this
process.
w = (?) kJ
q = (?) kJ
ΔH = (?) kJ
ΔS = (?) J/(mol*K)

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

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...

5 mole of an ideal gas for which Cv,m=3/2R, initially at 20 oC
and 1 atm undergoes a two-stage transformation.
For each of the stages described in the following list,
Calculate the final pressure as well as q, w, ∆U, ∆H and ∆S.
a) The gas is expanded isothermally and reversibly until the
volume triple.
b) then, the temperature is raised to T=2000 oC at the constant
volume. Note: R= 8.314 j/mol.K or 0.082 lt.atm/mol.K, 1lt.atm=
101.325 joule

32) 3.00 moles of an ideal gas are expanded isothermally
against a constant pressure of 1 atm from 2.0 liters to 10.0 liters
at a temperature of 20.0 C.
Which of the following is incorrect?
1. w = -PDV = -(1atm)(8 l) = -(101.3 J/l)(8 l) = -811.2 J
2. q = -w (since DU = 0) = 811.2 J
3. DU = 0 (since isothermal ideal gas)
4. DSSYS = ∆H/T = 0
33) In general, for a thermodynamic...

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