0.7 liters of an ideal gas is initially at atmospheric pressure. Process a-b: Th

ID: 1543780 • Letter: 0

Question

0.7 liters of an ideal gas is initially at atmospheric pressure.

Process a-b: The gas is allowed to expand isothermally to 1.8 liters.

Process b-c: The gas is returned to atmospheric pressure at constant volume.

Process c-d: The gas is returned to the initial volume, 0.7 liters, at constant pressure.

A) Process a-b: Determine the amount of work that was done.
(include units with answer)

B)Process a-b: Determine the change in internal energy.

C)Process a-b: Determine the heat that was added.

D)Process b-c: Determine the work that was done.

E)Process c-d: Determine the work that was done.

part A:

work done for isothermal expansion =pressure*volume*ln(final volume/initial volume)

=1 atm*0.7 ltr*ln(1.8/0.7)

=101325 Pa*0.0007*ln(1.8/0.7)

=66.988 J

part B:

change in internal eenrgy=0 as it is an isothermal process.

part c:

heat added=change in internal energy+work done=0+66.988=66.988 J

part d:

process b-c is a constant volume process.

hence work done=0

part e:

process c-d is a constant pressure process ..

work done=pressure*(final volume-initial volume)

=101325 Pa*(0.7-1.8) ltr

=101325*(-1.1)*0.001 m^3

=-111.46 J

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