Chemistry - Thermodynamics - I Question with Solution | TestHub

One mole of an ideal monoatomic gas $\left({\mathrm{C}}_{\mathrm{V},\mathrm{m}}=1.5\mathrm{R}\right)$ is subjected to the following sequence of steps :

(a) The gas is heated reversibly at constant pressure of 1 atm from 298 K to 373 K.

(b) Next, the gas is expanded reversibly and isothermally to double its volume.

(c) Finally, the gas is cooled reversibly and adiabatically to 308 K.

Calculate the net amount of heat (in J) absorbed in the overall process.

(R = 8.314 J/K-mol, ln2 = 0.70)