Question

An ideal gas at 300 K has a volume of 15 L at a pressure of 15 atm. Calculate the:

(1)the ﬁnal volume of the system,

(2) the work done by the system,

(3) the heat entering thesystem,

(4) the change in internal energy when the gas undergoes

a.- A reversible isothermal expansion to a pressure of 10 atm

b.- A reversible adiabatic expansion to a pressure of 10 atm.

Answer #1

Suppose 4.00 mol of an ideal gas undergoes a reversible
isothermal expansion from volume V1 to volume V2 = 8V1 at
temperature T = 300 K. Find (a) the work done by the gas and (b)
the entropy change of the gas. (c) If the expansion is reversible
and adiabatic instead of isothermal, what is the entropy change of
the gas?

A sample consisting of 2.5 moles of ideal gas (Cp,m
=20.8 J/K) is initially at 3.25 atm and 300 K. It undergoes
reversible adiabatic expansion until its pressure reaches 2.5 atm.
Calculate the final volume, the final temperature, and the work
done.

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.

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...

A 0.505-mol sample of an ideal diatomic gas at 408 kPa and 309 K
expands quasi-statically until the pressure decreases to 150 kPa.
Find the final temperature and volume of the gas, the work done by
the gas, and the heat absorbed by the gas if the expansion is the
following.
(a) isothermal
final temperature K
volume of the gas
L
work done by the gas
J
heat absorbed
J
(b) adiabatic
final temperature K
volume of the gas L...

A Joule expansion refers to the expansion of a gas from volume
V1 to volume V2 against no
applied pressure, and is sometimes also called a free expansion.
There is no work done, because the P of -PdV is
zero. By insulating the system, this process can be done
adiabatically, so there is no change in heat. For an ideal gas, the
adiabatic process is also isothermal, so there is no change in
thermodynamic energy, ∆U = 0 (which is...

2.)1.0 mol sample of an ideal monatomic gas originally at a
pressure of 1 atm undergoes a 3-step process as follows:
(i) It expands
adiabatically from T1 = 588 K to T2 = 389 K
(ii) It is compressed at
constant pressure until its temperature reaches T3 K
(iii) It then returns to its
original pressure and temperature by a constant volume process.
A). Plot these processes on a PV diagram
B). Determine the temperature T3
C)....

Thermodynamics Question
A Joule expansion refers to the expansion of a gas from volume
V1 to volume V2against no
applied pressure, and is sometimes also called a free expansion.
There is no work done, because the P of -PdV is
zero. By insulating the system, this process can be done
adiabatically, so there is no change in heat. For an ideal gas, the
adiabatic process is also isothermal, so there is no change in
thermodynamic energy, ∆U = 0 (which...

150 grams of C2H6 an ideal gas has an
initial pressure of 9120 mmHg and a temperature of 300 K. At a
constant temperature and moles, the gas changes to a final pressure
is 2280 mmHg.
a) Calculate the initial and final volumes (L)
b) Calculate the work done (in kJ) for the gas volume change if
it is carried out against a constant external pressure of 6 atm. (1
L atm = 101.325 J)
c) Using answer 5b, is...

An ideal monatomic gas is contained in a vessel of constant
volume 0.330 m3. The initial temperature and pressure of the gas
are 300 K and 5.00 atm, respectively. The goal of this problem is
to find the temperature and pressure of the gas after 24.0 kJ of
thermal energy is supplied to the gas.
(a) Use the ideal gas law and initial conditions to calculate
the number of moles of gas in the vessel. Your response differs
from the...

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