'n' moles of an ideal monoatomic gas has been expanded reversily isothermally at 300 K from 1 lit, 5 atm to 5 lit. and then it has been restored to it's initial position isothermally ag

Question

'n' moles of an ideal monoatomic gas has been expanded reversily isothermally at 300 K from 1 lit, 5 atm to 5 lit. and then it has been restored to it's initial position isothermally against a constant external pressure of 5 atm. Calculate entropy change (in $J / K$ ) in the surroundings during the entire process.

(Use : ln(5) = 1.6, 1 lit-atm = 100 J).

TestHub · Accepted Answer

Δ S s u rro u n d in g ​ = − 300 Δ Q sys , re v ​ ​ − 300 Δ Q i rr a ​ ​ = [ 300 − 5 l n ( 5/1 ) ​ − 300 5 ( 1 − 5 ) ​ ] = − 60 1 ​ [ ln 5 − 4 ] 60 2.4 ​ l i t − a t m k − 1 = 4 × 1 0 − 2 l i t − a t m k − 1

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