Question

2.25 moles of an ideal gas with Cv,m = 5R/2 are transformed
irreversibly from an initial

state T = 680 K and P = 1.15 bar to a final state T= 298 and P=
4.75 bar.

a) Calculate ΔU, ΔH, and ΔS for this process.

b) Calculate ΔU, ΔH, and ΔS for this process was reversible.

Answer #1

2.25 moles of an ideal gas with Cv,m = 5R/2 are transformed
irreversibly from an intital state T=680 K and P= 1.15 bar to a
final state T = 298 K and P = 4.75 bar a) Calculate change in
internal energy, change in enthalpy, and change in entropy for this
process b) Calculate change in internal energy, change in enthalpy,
and change in entropy if this process was reversible.

2.85 moles of an ideal gas with CV,m=3R/2 undergoes the
transformations described in the following list from an initial
state described by T = 310. K and P = 1.00 bar.
Part A:The gas is heated to 600 K at a constant volume
corresponding to the initial volume. Calculate q for this process.
Express your answer with the appropriate units.
Part B:The gas is heated to 600 K at a constant volume
corresponding to the initial volume. Calculate w for...

2.15 mol of an ideal gas with CV,m=3R/2
undergoes the transformations described in the following list from
an initial state described by T=350.K and
P=5.00bar.
1) The gas undergoes a reversible adiabatic expansion until the
final pressure is one-fourth its initial value.
2) The gas undergoes an adiabatic expansion against a constant
external pressure of 1.25 bar until the final pressure is
one-fourth its initial value.
3)The gas undergoes an expansion against a constant external
pressure of zero bar until...

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.

a. One mole of an ideal monoatomic gas (closed system, Cv,m)
initially at 1 atm and 273.15 K experiences a reversible process in
which the volume is doubled. the nature of the process is
unspecified, but the following quantities are known, deltaH=2000.0J
and q=1600.0J. Calculate the initial volume, the final temperature,
the final pressure, deltaU, and w for the process.
b. Suppose the above gas was taken from the same initial state
to the same final state as in the...

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

6. An ideal
monatomic gas initially at 26.85 K and 3.250 bar is added to a
1.750 L vessel. Assuming that the system consists of the ideal gas
alone, calculate the values of Vf, Tf, Pf, w, q, ΔU, and ΔH for
each of the following processes. Construct a table for each part
listing the initial and final value of V, T, and P and the value of
w, q, ΔU, and ΔH.

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).

Initially 5.00 mol of neon gas (CV =
3R/2 and γ = 5R/2) are at absolute
temperature 305 K and occupy volume 4.00×10−2m3. Then the gas
expands adiabatically to a new volume of 9.00×10−2m3.
A) Calculate the initial pressure of the gas.
B) Calculate the final pressure of the gas.
C) Calculate the final temperature of the gas.
D) Calculate the work done as the gas expands.

1)
A quantity of n moles of oxygen gas
(CV = 5R/2 and Cp =
7R/2) is at absolute temperature T. You increase
the absolute temperature to 2T. Find the change in
internal energy of the gas, the heat flow into the gas, and the
work done by the gas if the process you used to increase the
temperature is isochoric.
Express your answers in terms of the variables n,
R, and T separated by commas.
2)
Find the change...

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