Question

In this problem, 1.10 mol of an ideal gas at 300 K undergoes a free adiabatic expansion from V1 = 12.3 L to V2 = 22.2 L. It is then compressed isothermally and reversibly back to its original state.

(a) What is the entropy change of the universe for the complete
cycle?

J/K

(b) How much work is lost in this cycle?

J

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?

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?

Ideal gas ethylene undergoes a reversible adiabatic compression
by which its temperature increases from T1 = 300 K to T2 = 450 K.
The molar entropy in the initial state is given as s1 = 100 J K–1
mol–1, and here, for ethylene, cp = ?T + c0 with ? = 0.1 J K–2
mol–1 and c0 = 13.1 J K–1 mol–1. Determine the change of the molar
entropy s2 – s1 and the change of the chemical potential ?2...

A sample of 64.0 g of methane, CH4 (molecular mass
16.0 g/mol, assume ideal gas behaviour)) at 300 K and with an
initial pressure V1 = 1.00 m3 is
compressed isothermally and reversibly to a final volume
of 2.00L. Calculate DU, DH, w, and q

Calculate q and w for a process where 1.7 mol of an ideal gas at 300 K is isothermally and reversibly compressed from the pressure of 1.5 bar to 2.5 bar. Also enter the sign of the calculated q and w value and what it means. (heat delivered or absorbed and work done or required)

3. Two moles of an ideal gas
at an initial temperature of 400 K are confined to a volume of 40.0
L. The gas then undergoes a free expansion to twice its
initial volume. The container in which this takes place
is insulated so no heat flows in or out. (1 Liter =
10-3
m3) R = 8.314 J/(mole
K)
a) What is the entropy change
of the gas? (15 points)
b) What is the entropy change
of the universe? (10 points)

A cylinder contains an ideal gas at the temperature of 300 K and
is closed by a movable piston. The gas, which is initially at a
pressure of 3 atm occupying a volume of 30 L, expands isothermally
to a volume of 80 L. The gas is then compressed isobarically,
returning to its initial volume of 30 L. Calculate the work done by
gas: a) in isothermal expansion; b) in isobaric compression, c) in
the whole process; and d) Calculate...

Use these steps to answer the questions below:
Step 1: A sample of monoatomic ideal gas, initially at pressure
P1 and volume V1, expands isothermally and
reversibly to a final pressure P2 and volume
V2
Step 2: The ideal gas is compressed isothermally back to its
initial conditions using constant pressure.
Give the equation needed to solve for the following
Wsys (Step 1)
=
qsys (Step 2)
=

An ideal gas with γ = 1.4 occupies 6.0 L at 300 K and 100 kPa
pressure. It is compressed adiabatically until its volume is 2.0 L.
It's then cooled at constant pressure until it reaches 300 K, then
allowed to expand isothermally back to its initial state.
a.) Find the net work done on the gas.
b.) Find the minimum volume reached.

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.

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