Question

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.

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...

One mole of an ideal gas expands reversibly and isothermally
from 10. bar to 1.0 bar at 298.15K.
(i)Calculate the values of w, q, ∆U and ∆H?
(ii)Calculate w if the gas were to have expanded to the same
final state against a constant pressure of 1 bar.

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 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.

A two mole sample of an ideal diatomic gas expands
slowly and adiabatically from a pressure of 5 atm. and a volume of
10 liters up to a final volume of 30 liters.
a) What is the final pressure of the gas ?,
b) Whatis the heat, work and internal energy?

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

One gram-mole of ideal gas is contained in a piston-cylinder
assembly. Cp=(7/2)R, Cv=(5/2)R. The gas expands from 3 to 1 atm.
Heat of 1000J is transferred to the gas during the process.
External pressure maintains at 1 atm throughout. Initial
temperature of the gas is 300K. Find work and internal energy
change.

One mole of an ideal gas initially at a temperature of
Ti = 5.6°C undergoes an expansion at a constant
pressure of 1.00 atm to nine times its original volume.?
(a) Calculate the new temperature
Tf of the gas.
_____ K
(b) Calculate the work done on the gas during the
expansion.?
_____kJ

One mole of an ideal gas initially at a temperature of
Ti = 7.6°C undergoes an expansion at a constant
pressure of 1.00 atm to three times its original volume.
(a) Calculate the new temperature
Tf of the gas.
K
(b) Calculate the work done on the gas during the
expansion.
kJ

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