Question

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?

Answer #1

A 2.00-mol sample of a diatomic ideal gas expands slowly and
adiabatically from a pressure of 5.04 atm and a volume of 13.0 L to
a final volume of 31.0 L.
(a) What is the final pressure of the gas?
atm
(b) What are the initial and final temperatures?
initial
K
final
K
(c) Find Q for the gas during this process.
kJ
(d) Find ΔEint for the gas during this
process.
kJ
(e) Find W for the gas during...

One
mole of an ideal gas at 25 degrees celsius and one atmosphere
pressure expands adiabatically to twice its original volume, then
compresses isothermally back to the original volume, then proceeds
isochorically back to the initial conditions. How much work is done
by the gas?
work done by the ideal gas.

An ideal gas with γ = 1.400 expands adiabatically from a
pressure of 365.0 Pa and a volume of 70.00 m3 , doing 101.0 J of
work while expanding to a final volume. What is its final
pressure-volume product?

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 0.520-mol sample of an ideal diatomic gas at 432 kPa and 324 K
expands quasi-statically until the pressure decreases to 144 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 and adiabatic final temperature volume of the gas
wrok done by the gas heat absorbed?
K=?, L=?, work done?, heat absorb?

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...

2.50 mol of a diatomic ideal gas expands adiabatically and
quasi-statically. The initial temperature of the gas is 325 K. The
work done by the gas during expansion is 7.50 kJ.
(a) What is the final temperature of the gas?
K
(b) Compare your result to the result you would get if the gas
were monatomic. (Calculate the final temperature if the gas were
monatomic.)
K

The volume of an ideal gas is adiabatically reduced from 200 L
to 74.3 L. The initial pressure and temperature are 1.00 atm and
300 K. The final pressure is 4.00 atm.
? = 8.314 J/mol.K , ????????? = 1.4, ??????????? = 1.67 and 1
atm = 1.013 × 10^5 Pa. mol.K
(a) Is the gas monatomic or diatomic?
(b) What is the final temperature?
(c) How many moles are in 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...

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