Five moles of an ideal gas at - 300K- expanded isothermally from an initial pressure of - 4 atm- to a final pressure of 1 atm against a cont- external the pressure of - 1 atm- Calculate - q- w- - - U- amp- - - H- Calculate the corresponding value of all if the above process is carried out reversiblyNone of these- w-irr - 9356-25 J- w-rev - 17291-6 J- - U - - H - 0- w-irr - -9356-25 J- w-rev - 17291-6 J- - U - - H - 0- w-irr - 9356-25 J- w-rev - -17291-6 J- - U - - H - 0-

The correct option is B w_irr = 9356.25 J, w_rev = 17291.6 J, Δ U = Δ H = 0 W_irr= nRT (1 P_2/P_1 )= 5× 8.314× 300 (1 1/4 ) W_irr= 9.353 kJ ...

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Calorimetry

Five moles of...

Question

Five moles of an ideal gas at $300 K$ , expanded isothermally from an initial pressure of $4 a t m$ to a final pressure of 1 atm against a cont. external the pressure of $1 a t m$ . Calculate $q, w,$ $Δ U$ & $Δ H$ . Calculate the corresponding value of all if the above process is carried out reversibly

w_{i r r} = 9356.25 J, w_{r e v} = 17291.6 J, Δ U = Δ H = 0

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w_{i r r} = - 9356.25 J, w_{r e v} = 17291.6 J, Δ U = Δ H = 0

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w_{i r r} = 9356.25 J, w_{r e v} = - 17291.6 J, Δ U = Δ H = 0

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None of these

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