Question

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

Answer #1

where *dU* is the change in the internal energy of the
system and *?W* is work done *by* the system. Any
work (*?W*) done must be done at the expense of internal
energy *U*, since no heat *?Q* is being supplied from
the surroundings. Pressure-volume work *?W* done *by*
the system is defined as

It is desired to know how the values of *dP* and
*dV* relate to each other as the adiabatic process proceeds.
For an ideal gas the internal energy is given by

a)

7.5*1000=1.4*2.5*8.314(T-325)

T=582.74k

b)

7.5*1000=1.66*2.5*8.314*(T-325)

T=542.37K

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Find the final temperature and volume of the gas, the work done by
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(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...

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1. An ideal monatomic gas, with 24.05 moles, expands
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Specify whether the change is an increase or a decrease.

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? = 8.314 J/mol.K , ????????? = 1.4, ??????????? = 1.67 and 1
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A vessel with a movable piston contains 1.90 mol of an ideal gas
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Pi = 2.03 ✕ 105 Pa,
initial volume
Vi = 1.00 ✕ 10−2
m3,
and initial temperature
Ti = 128 K.
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J
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J
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An ideal monatomic gas is contained in a vessel of constant
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