Question

- One mole of a monoatomic, ideal gas at initial pressure
*P*and volume_{0}*V*goes to 2_{0}*P*a) along the path_{0}*PV =*constant, and b) at constant volume. Find the heat added to the gas in each case.

Answer #1

One mole of a monoatomic, ideal gas at initial pressure
P0 and volume V0 goes to
2P0 a) along the path PV = constant,
and b) at constant volume. Find the heat added to the gas in each
case.

One mole of a monoatomic, ideal gas at initial pressure
P0 and volume V0 goes to
2P0 a) along the path PV = constant,
and b) at constant volume. Find the heat added to the gas in each
case.

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.

One mole of an ideal gas at atmospheric pressure expands
isobarically from a volume of 1m3 to a volume of
2m3.
1 - Find the initial and final temperatures of the gas
2 - Find the work done by the gas
3 - Find the heat added to the gas

A mole of a monatomic ideal gas is taken from an initial
pressure p and volume V to a final pressure 3p and volume 3V by two
different processes: (I) It expands isothermally until its volume
is tripled, and then its pressure is increased at constant volume
to the final pressure. (II) It is compressed isothermally until its
pressure is tripled, and then its volume is increased at constant
pressure to the final volume. Show the path of each process...

The diagram shows the pressure and volume of an ideal gas during
one cycle of an engine. (Figure 1) As the gas proceeds from state 1
to state 2, it is heated at constant pressure. It is then cooled at
constant volume, until it reaches state 3. The gas is then cooled
at constant pressure to state 4. Finally, the gas is heated at
constant volume until it returns to state 1.
Part A
Find W12 , the work done...

. A container has n = 3 moles of a monoatomic ideal gas at a
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isochorically (constant volume) to half of the initial value. 3.-
The gas is compressed isobarically back to its initial volume. 4.-
The...

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
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independent of temperature. Calculate the work done, the heat
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carried out
(1) isothermally and reversibly, and
(2) adiabatically and reversibly.
Having determined the final state of the...

After a free expansion to increase its volume by a factor of
seven, a mole of ideal diatomic gas is compressed back to its
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final step to restoring its original state? (Use the following as
necessary: p0 for the initial pressure and V0 for the initial
volume.)

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.

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