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 changes 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 changes 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> :<a href="https://interviewquestions.tuteehub.com/tag/pressure-1164240" style="font-weight:bold;" target="_blank" title="Click to know more about PRESSURE">PRESSURE</a> of an ideal gas =`P_i` = 4.1 atm. <br/> <a href="https://interviewquestions.tuteehub.com/tag/expansion-980011" style="font-weight:bold;" target="_blank" title="Click to know more about EXPANSION">EXPANSION</a> in volume `DeltaV` = 2 litres <br/> Heat absorbed =<a href="https://interviewquestions.tuteehub.com/tag/q-609558" style="font-weight:bold;" target="_blank" title="Click to know more about Q">Q</a> = 3710 J <br/>Entropy change = `DeltaS` = ?<br/>For an ideal gas PV = RT for one mole . <br/> `T=(PV)/<a href="https://interviewquestions.tuteehub.com/tag/r-611811" style="font-weight:bold;" target="_blank" title="Click to know more about R">R</a>=(4.1xx2)/0.0830=100^@C` <br/> T=100+273 = 373 K <br/>`DeltaS=q/T_((K))=3710/373` <br/> Entropy change =9.946 `JK^(-1)`</body></html>