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One moles of an ideal gas which C(V) = 3...

One moles of an ideal gas which `C_(V) = 3//2 R` is heated at a constant pressure of `1 atm` from `25^(@)C` to `100^(@)C`. Calculate `DeltaU, DeltaH` and the entropy change during the process.

A

223.5 cal an d372.56 cal

B

356.76 cal and 356.46 cal

C

437.3 cal and 357.76 cal

D

396.5 cal and 436.5 cal

Text Solution

Verified by Experts

As `(C_(p) - C_(V))=R rArr C_(p) = C_(v) +R`
`rArr C_(p) = 3/2 R +R = 5/2 R`
Heat given at constant pressure
`(DeltaH) = nC_(p) DeltaT = 1 xx 5/2 R xx (373 - 298)`
`rArr DeltaH = 1 xx 5/2 xx 1.987 xx 75 = 372.56` cal
Work done in the process = `-PDeltaV`
`=-P(V_(2) - V_(1)) = -P((nRT_(2))/P - (nRT_(1))/P)` (As PV = nRT)
`-nR(T_(2)-T_(1)) = -1 xx 1.987 xx (373 - 298) = 149.05 cal`
From first law of thermodynamics.
`DeltaE = q-W = 372.56 - 149.05 = 223.51` cal
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