Question

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

Answer #1

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

A 2.5 mol sample of ideal gas initially at 1 atm and 25 °C is
expanded isothermally (ΔT = 0) and reversibly to twice its original
volume.
What is the change in internal energy?

3.75 moles of ideal fas with CV,m=3/2R undergoes the
transformations described in the following list from an initial
state described by T=298K and P=4.50 bar.
c)The gas undergoes an expansion against a constant external
pressure of zero bar until the final pressure is one third its
initial value. Find S

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.

Assume that one mole of a monatomic (CV,m = 2.5R) ideal gas
undergoes a reversible isobaric expansion at 1 bar and the volume
increases from 0.5 L to 1 L. (a) Find the heat per mole, the work
per mole done, and the change in the molar internal energy, ΔUm,
the molar enthalpy, ΔHm, for this process. b) What are the entropy
changes ΔSm of the system and of the surroundings? Is this process
spontaneous? Justify your answer.

Consider 1.00 mol of an ideal gas (CV = 3/2 R)
occupying 22.4 L that undergoes an isochoric (constant volume)
temperature increase from 298 K to 342 K. Calculate ∆p, q , w, ∆U,
and ∆H for the change.
For Units, pressure in atm and the rest in J.

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
Joules.

) An ideal gas (Cp = 5 kcal/kmol, Cv = 3
kcal/kmol) is changed from 1 atm and 22.4 m3 to 10 atm
and 2.24 m3 by the following reversible process
(i) Isothermal
compression
(ii) Adiabatic
compression followed by cooling at constant volume
(iii) Cooling at
constant pressure followed by heating at constant volume
Calculate the heat, work requirement,
?U and ?H for each
process.

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