In
an experiment, 1.35 mol of
oxygen
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Solution: Click For PDF Version Let the initial volume of the gas be and
its pressure be
The initial temperature of the gas is
 As the amount of oxygen gas is 1.35 mol, using the ideal gas equation of state we find
As the volume of the gas is doubled at constant pressure, the final temperature of the gas will be
For a diatomic gas the internal energy of n mol at temperature T is
therefore, the change in the internal energy of the gas on heating will be
We next calculate the work done on the gas during its expansion of its volume from V to 2V. It is given by
The fist law of thermodynamics states that
where Q is the heat energy supplied to the system during its change of state. Therefore,
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are heated at constant pressure starting at
.
We have to calculate the amount of heat that must be added to the gas
to double its volume.
