Question

Two moles of an ideal gas are expanded
Isothermally and reversibly from a volume.
of 15.5 l to a volume of 20 l against
constant external presure
I bar
estimate the amount
of
work done in Joule

Answer 1

Answer:

Two moles of an ideal gas are expanded isothermally from a volume of 15.5l to the volume of 20l against a constant external pressure of 1 atm estimate

Explanation:

Calculate the work done in L atm and joules. (-4.18 L atm ... V= initial volume=300cm ^3=0.3L P is constant external pressure=1.9atm

Answer 2

Given: Number of moles = 2

           Initial  volume = 15.5 L

           Final volume = 20L

To find: Work done in Joule

Solution: When an ideal gas is kept in a container and the gas expands isothermally and isobaric, then the work done by the gas is equal to the product of pressure, and change in volume of gas in a container.

• To say that work is done, the volume of the gas must change.

W = PdV ( At constant pressure)

W = Pext(Vf - Vi)

Where Pext is the external pressure applied, Vf is the final volume of the gas, Vi is the initial volume of the gas.

W = 1 (20-15.5)

   = 1 (0.5)

   = 0.5 barL

As 1 barL is equal to 100 Joule

Therefore, 0.5 barL is equal to 50 Joule

Therefore, 50 Joule of work is done when a gas expands from 15.5L to 20L against external pressure 1 bar.