Two moles of an ideal monoatomic gas at 5 bar and 300K are expanded adiabatically, irreversibly up to an external pressure of text1 bar. The work is done by the gas is -xR (in bar.Litre). The value of x is [ R is gas constant]

Question

Two moles of an ideal monoatomic gas at 5 bar and 300K are expanded adiabatically, irreversibly up to an external pressure of text1 bar. The work is done by the gas is -xR (in bar.Litre). The value of x is [ R is gas constant] (A)  (B)  (C)  (D)

Tardigrade Admin · Accepted Answer

Given: pf i n a l=pe x t so p1=5 , p2=1 and pe x t=1 , T1=300,T2=? for the calculation of T2 nCv(T2 - T1)=-pe x t(V2 - V1)=-pe x t[(n R T2/P2) - (n R T1/P1)] nCv(T2 - T1)=-pe x t[(n R T2/P2) - (n R T1/P1)] nCv(T2 - T1)=-pe x t[(n R T2/P2) - (n R T1/P1)] Cv(T2 - T1)=pe x t[(R T2/P2) - (R T1/P1)] ((3 R/2))(.T2 -300.)=-1[(R × T2/1) - (R × 300/5)] textT text2 text= text204 textK Wi r r , a d i a=-1[(2 × R × 204/1) - (2 × R × 300/5)] =-288 R

Q. Two moles of an ideal monoatomic gas at 5 bar and 300K are expanded adiabatically, irreversibly up to an external pressure of 1 bar. The work is done by the gas is −xR (in bar.Litre). The value of x is [ R is gas constant]

Q. Two moles of an ideal monoatomic gas at $5$ bar and $300 K$ are expanded adiabatically, irreversibly up to an external pressure of $1$ bar. The work is done by the gas is $- x R$ (in bar.Litre). The value of $x$ is [ $R$ is gas constant]