Question

One mole of an ideal gas at 300 K is expanded adiabatically and reversibly from 20 atm to 1 atm. What is the final temperature of the gas, assuming Cv= 3/2R.

Question 1 options: a) 400 K b) 250 K c)156 K d)90.5 K

Answer #1

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.

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?

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

Five kilograms of steam initially at 1.40 MPa and 650 °C are
reversibly and adiabatically expanded to Tsat= 40 °C.
Determine the quality of the steam in its final state and the work
required.
(Cp=33.59 J/mole-K CV=25.275 J/mole-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...

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 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.

The volume of an ideal gas is adiabatically reduced from 217 L
to 65.6 L. The initial pressure and temperature are 1.70 atm and
300 K. The final pressure is 9.07 atm. (a) Is the
gas monatomic, diatomic, or polyatomic? (b) What
is the final temperature? (c) How many moles are
in the gas?

The volume of an ideal gas is adiabatically reduced from 200 L
to 74.3 L. The initial pressure and temperature are 1.00 atm and
300 K. The final pressure is 4.00 atm.
? = 8.314 J/mol.K , ????????? = 1.4, ??????????? = 1.67 and 1
atm = 1.013 × 10^5 Pa. mol.K
(a) Is the gas monatomic or diatomic?
(b) What is the final temperature?
(c) How many moles are in the gas?

1. A sample of 1.00 mol of an ideal gas at 27oC and 1.00 atm is
expanded adiabatically and reversibly to 0.50 atm. Determine the
values of Tf, q, w, deltaU, deltaH, deltaS, deltaG,
deltaSsurr and deltaStot. Take Cv = 3/2
R.

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