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One-mole-of-steam-is-condensed-at-100-C-the-water-is-cooled-to-0-C-and-frozen-to-ice-Which-of-the-following-statements-are-correct-given-heat-of-vapourization-and-fusion-are-540-cal-gm-and-80-cal-




Question Number 23864 by Tinkutara last updated on 08/Nov/17
One mole of steam is condensed at  100°C, the water is cooled to 0°C and  frozen to ice. Which of the following  statements are correct, given heat of  vapourization and fusion are 540 cal/  gm and 80 cal/gm? (average heat  capacity of liquid water = 1 cal gm^(−1)   degree^(−1) )  (1) Entropy change during the  condensation of steam is −26.06 cal/°C  (2) Entropy change during cooling of  water from 100°C to 0°C is −5.62 cal/°C  (3) Entropy change during freezing of  water at 0°C is −5.27 cal/°C  (4) Total entropy change is −36.95  cal/°C
Onemoleofsteamiscondensedat100°C,thewateriscooledto0°Candfrozentoice.Whichofthefollowingstatementsarecorrect,givenheatofvapourizationandfusionare540cal/gmand80cal/gm?(averageheatcapacityofliquidwater=1calgm1degree1)(1)Entropychangeduringthecondensationofsteamis26.06cal/°C(2)Entropychangeduringcoolingofwaterfrom100°Cto0°Cis5.62cal/°C(3)Entropychangeduringfreezingofwaterat0°Cis5.27cal/°C(4)Totalentropychangeis36.95cal/°C
Answered by ajfour last updated on 09/Nov/17
All correct (I believe).       ∫dS = ∫ (dQ/T) .  during conensation  T=373K  (constant)  ∫dQ=−mL_(vap)   So   △S_(condensation) =−((18×540)/(373)) (J/K)      =−26.06 J/K  △S_(cooling) =∫_(373) ^(  273)   ((mc dT)/T)     =−18ln (((373)/(273))) ≈ −18ln (((124.3)/(91)))     ≈−18×2.303×(3log 5−2log 3−1)     ≈ −18×2.3×[3(1−0.3010)−2×0.4771−1]  ≈ −18×2.3[2.1−1.9542]  ≈ −18×2.3×0.145  ≈ −9×2.3×0.29= 20.7×0.29 J/K      ≈−6 J/K .  △S_(freezing) =−((mL_(fusion) )/T_f )            =((−18×80)/(273)) = −5.27 J/K  △S_(net) =−(26+6+5.3)J/K              =−37.3 J/K .
Allcorrect(Ibelieve).dS=dQT.duringconensationT=373K(constant)dQ=mLvapSoScondensation=18×540373JK=26.06J/KScooling=373273mcdTT=18ln(373273)18ln(124.391)18×2.303×(3log52log31)18×2.3×[3(10.3010)2×0.47711]18×2.3[2.11.9542]18×2.3×0.1459×2.3×0.29=20.7×0.29J/K6J/K.Sfreezing=mLfusionTf=18×80273=5.27J/KSnet=(26+6+5.3)J/K=37.3J/K.
Commented by Tinkutara last updated on 09/Nov/17
Why in calculating ΔS_(condensation) and  ΔS_(freezing)  you have taken them to be  −mL? Why not +mL? I know that  entropy decreases but in formula  there is only + sign.
WhyincalculatingΔScondensationandΔSfreezingyouhavetakenthemtobemL?Whynot+mL?Iknowthatentropydecreasesbutinformulathereisonly+sign.
Commented by Tinkutara last updated on 10/Nov/17
Thank you very much Sir!
ThankyouverymuchSir!
Commented by ajfour last updated on 09/Nov/17
dQ is heat received by system;  and during freezing or during  condensation heat is given out  by the system so ∫dQ =−∣mL∣ .
dQisheatreceivedbysystem;andduringfreezingorduringcondensationheatisgivenoutbythesystemsodQ=mL.

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