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 A total `1000 J` of heat is withdrawn from the sample of the cyclic process .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`.
Which graph between temperature `T` and volume `V` for the cyclic process is correct.

Options

A. ` (##BMS_V06_C02_E01_249_O01.png" width="30%">
B. ` (##BMS_V06_C02_E01_249_O02.png" width="30%">
C. ` (##BMS_V06_C02_E01_249_O03.png" width="30%">
D. ` (##BMS_V06_C02_E01_249_O04.png" width="30%">

Answer

C

Explanation

An `AB` is isobaric, in `B rarr C` magnitude of `(dT)/( dv)` increases and `OA` is isochoric process.