Two moles of triatomic linear gas are taken through a reversible process staring from `A` as shown in figure. The volume ratio `(V_(B))/(V_(A)) = 4`. If the temperature at 'A' is `-73^(@)C` then determine total enthalpy change in both steps.
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The correct Answer is:
B
Two moles of traiatomic linear gas ………… `Delta H_(total) = Delta H_(AB)+Delta H_(BC)` `=nC_(p)Delta T + 0` `= 2xx(7)/(2)xxRxx(800-200)` `= 4200 R`
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