Four moles of an ideal gas is initially in state `A` having pressure ` 2 xx 10^(5) N//m^(2)` and temperature ` 200 K` . Keeping the pressure constant the gas is taken to state `B` at temperature of `400K`. The gas is then taken to a state `C` in such a way that its temperature increases and volume decreases. Also from `B` to `C` , the magnitude of `dT//dV` increases. The volume of gas at state `C` is eqaul to its volume at statem `A`. Now gas is taken to initial state `A` keeping volume constant. A total `1000 J` of heat is withdrawn from the sample of the cyclic process . Take `R=8.3 J// K// mol`. The volume of gas at state `C` is

Options

A. `0.0332 m ^(3)`
B. `0.22 m^(3)`
C. `0.332m ^(3)`
D. `3.32 m ^(3)`

Answer

A

Explanation

The volume of gas at state `C` is
`V_(C)=V_(A)=(nRT_(A))/(P_(A))`
`=0.0332m^(3)`