Question

Consider one mole of air with initial temperature of 0 degrees Celicus and pressure of 1000 mb. The air undergoes a polytropic process, with its volume expanded 3 times at 250 mb. Calculate:

(a) The power n of the polytropic process;

(b) The final temperature;

(c) The change of internal energy, the work done on, and the heat absorbed by the system.

Answer #1

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...

1 mole of a gas undergoes a mechanically reversible isothermal
expansion from an initial volume 1 liter to a final volume 10 liter
at 25oC. In the process, 2.3 kJ of heat is absorbed in the system
from the surrounding. The gas follows the following formula:
V=RTP+b where V is the molar specific volume, and Tand Pare
temperature (abosolute) and gas pressure respectively. Given R=
8.314 J/(mol.K) and b= 0.0005 m3. Evaluate the following a) Work
(include sign) b) Change...

Air at 1 atm and 20 0C occupies an initial volume of 1000 cm3 in
a cylinder. The air is confined by a piston which has a constant
restraining force so that the gas pressure always remains constant.
Heat is added to the air until its temperature reaches 260 0C.
Calculate (a) the heat added (b) the work done by the gas, (c) the
change in internal energy of the gas.

One mole of air is compressed from pressure P1 and temperature
T1 at
constant volume till its pressure is doubled. Then it is
expanded
reversibly and isothermally to the original pressure, and finally
restored
to the original temperature by cooling at constant pressure. Sketch
the
path followed by the gas, on a P-V diagram and calculate the net
work
done by the gas.

A) 1 kg of air with a pressure of 13 bar and a temperature of
125 ° C is heated as isobar up to 550 ° C.
a) Work done during heating,
b) Internal energy and enthalpy change,
c) Calculate the amount of heat consumed. (R = 287 j / kgK, x =
1,4)
B) An ideal gas with a pressure of 1 bar and a volume of 0.5m³
is compressed isothermally up to 17 bar pressure. Calculate the
volume...

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.

In an isobaric process if the the initial volume of air
is 2.3 litres at a temperature of 15°C and a pressure of 55kPa. If
the final temperature is 190° C
a) The final volume
b) The mass of air
c) The work done
d) The heat transferred

A gas contained in a closed rigid container is heated from
initial temperature and pressure of 270C and 2 bar to a
final pressure of 12 bar. Calculate final temperature, Work done,
Heat transfer and change in Internal Energy. (Take
Cv as 0.873 kJ/kg K. and Mass of the gas =
1kg)

Assume that one mole of a monatomic (CV,m = 2.5R) ideal gas
undergoes a reversible isobaric expansion at 1 bar and the volume
increases from 0.5 L to 1 L. (a) Find the heat per mole, the work
per mole done, and the change in the molar internal energy, ΔUm,
the molar enthalpy, ΔHm, for this process. b) What are the entropy
changes ΔSm of the system and of the surroundings? Is this process
spontaneous? Justify your answer.

Oxygen gas is contained in a piston cylinder assembly at an
initial pressure of 1000 kPa and expands from 0.2 m3 to 1.0 m3 by a
process where PV = constant. The gas has an internal energy change
of -200 kJ. Calculate the work (kJ) and the heat transfer (kJ) done
during the process.

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