Question

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

Answer #1

Suppose 0.540 mol of an ideal gas is isothermally and reversibly
expanded in the four situations given below. What is the change in
the entropy of the gas for each situation?
Situation (a) (b) (c) (d)
Temperature (K) 250 350 400 450
Initial volume (cm3) 0.200 0.200 0.450 0.350
Final volume (cm3) 0.900 0.700 1.20 1.25
deltaS (J/K) _____ _____ _____ _____

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

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 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 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 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 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 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?

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.

12 moles of a gas is compressed isothermally and reversibly from
400 K , 1 bar to 1/2th of its original volume. Initial
volume of the gas was measured at 120 cm^3. Using the truncated
virial EOS, calculate the required work for the compression.

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