Four moles of an ideal gas is initially in a state A having pressure `2xx10^(5)N//m^(2)` and temperature 200 K . Keeping 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 eaual to its volume at state A. Now gas is taken is initial state A keeping volume constant. A total of 1000 J heat is rejected from the sample in the cyclic process. Take `R=8.3J//K//mol`.
Which graph between temperture 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.