Calculate the boiling point of water at `24` torr pressure. The average `DeltaH_(vap.)` over the temperature range is `10.12 kcal mol^(-1)`. Will all the water form gaseous state if placed in a closed container, if not then, how wer can convert all the water into vapour state?

Explanation

`T_(bH_(2)O)=373 K` at `P=760 ` torr
`:' 2.303"log"(P_(2))/(P_(1))=(DeltaH)/R ([T_(2)-T_(1)])/(T_(1)T_(2))`
`:. 2.303 "log"(760)/(24)=(10.12xx10^(3))/2xx([373-T_(1)])/(373xxT_(1))`
`T_(1)=298 K =25^(@)C`
To make water boil at `25^(@)C`, it must be placed in closed container from which air is pumped until the pressure of the gas phase is is `24` torr. if all the water is to be boiled at `25^(@)C` continous pumping must be applied so that gas pressure is maintained at `24` torr.