The latent heat of vaporisation of water at `100 ^(@)C` is `540 cal g^(-1)`. Calculate the entropy increase when one mole of water at `100^(@)C` is ev
The latent heat of vaporisation of water at `100 ^(@)C` is `540 cal g^(-1)`. Calculate the entropy increase when one mole of water at `100^(@)C` is evaporated
A. `26 cal K^(-1) mol^(-1)`
B. `1.82 cal K^(-1) mol^(-1)`
C. `367 cal K^(-1) mol^(-1)`
D. `540xx18 cal K^(-1) mol^(-1)`
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Correct Answer - A
`DeltaS=(DeltaH_(vap))/(T)=(540xx18)/(373)`
`=26 cal K^(-1) mol^(-1)`
`(DeltaH_(vap) "for" 1 "mole"=540xx18)`
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