1 mole of an ideal gas, maintained at 4.1 atm and at a certain temperature, absorbs heat 3710 J and expands to 2 litres. Calculate the entropy change in expansion process.

1 mole of an ideal gas, maintained at 4.1 atm and at a certain tempera

1.	1 mole of an ideal gas, maintained at 4.1 atm and at a certain temperature, absorbs heat 3710 J and expands to 2 litres. Calculate the entropy change in expansion process.
Answer» <html><body><p></p><a href="https://interviewquestions.tuteehub.com/tag/solution-25781" style="font-weight:bold;" target="_blank" title="Click to know more about SOLUTION">SOLUTION</a> :`n=<a href="https://interviewquestions.tuteehub.com/tag/1-256655" style="font-weight:bold;" target="_blank" title="Click to know more about 1">1</a>"mole"` <br/> `P=4.1atm` <br/> `V=2" <a href="https://interviewquestions.tuteehub.com/tag/lit-537267" style="font-weight:bold;" target="_blank" title="Click to know more about LIT">LIT</a>"` <br/> `T=?` <br/> `q=3710J` <br/> `DeltaS=(q)/(T)` <br/> `DeltaS=(q)/(((PV)/(<a href="https://interviewquestions.tuteehub.com/tag/nr-581903" style="font-weight:bold;" target="_blank" title="Click to know more about NR">NR</a>)))` <br/> `DeltaS=(nRq)/(PV)` <br/> `DeltaS=(1xx0.082" lit atm "<a href="https://interviewquestions.tuteehub.com/tag/k-527196" style="font-weight:bold;" target="_blank" title="Click to know more about K">K</a>^(-1)xx3710J)/(4.1" atm"xx2" lit")` <br/> `DeltaS=37.10JK^(-1)`.</body></html>