Question

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.

Answer #1

The temperature is constant in an isothermal process

a)

b) For an isothermal process either reversible or irreversible the internal energy change, delta U is equal to zero (U=0)

c) From the first law of thermodynamics, U=Q+W

Q = -W =

d)

e)

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 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).

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.

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)

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

One mole of an ideal gas with is compressed adiabatically in a
single stage with a constant opposing pressure equal to 10atm.
pressure is 10 atm. Calculate the final temperature of the gas, w,
q, ΔU and ΔH. HINT – this is not reversible expansion.

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?

Ten liters of a monoatomic ideal gas at 25o C and 10
atm pressure are expanded to a final pressure of 1 atm. The molar
heat capacity of the gas at constant volume, Cv, is 3/2R and is
independent of temperature. Calculate the work done, the heat
absorbed, and the change in U and H for the gas if the process is
carried out
(1) isothermally and reversibly, and
(2) adiabatically and reversibly.
Having determined the final state of the...

You have a balloon consisting of Helium, which is
expanded isothermally at 25 ºC from
22.9 dm3
to 32.7 dm3
(i) reversibly, (ii) against a constant external pressure equal to
the
final pressure of the gas, and (iii) freely against zero external
pressure. Determine the work
(w). Please refer to Table Q2(b) for the number of moles of
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number of mole of helium = 16

5 moles of a monatomic ideal gas initially at 1 atm and 200 K is
compressed isothermally against a constant external pressure of 2.0
atm, to a final pressure of 2.0 atm. Calculate W; Q; U; and H in
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