Consider a saturated solution formed when 17.5 g of a solute dissolve in 28.3 g of a solvent, giving a total solution volume of
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Answer : The enthalpy change for converting 1 mole of ice at to water at
is, 7.712 KJ
Solution :
Process involved in the calculation of enthalpy change :
Now we have to calculate the enthalpy change.
where,
= enthalpy change
m = mass of water =
= specific heat of ice = 2.09 J/gk
= specific heat of water = 4.18 J/gk
= enthalpy change for fusion = 6.01 KJ/mole = 0.00601 J/mole
conversion :
= initial temperature of ice =
= final temperature of ice =
= initial temperature of water =
= final temperature of water =
Now put all the given values in the above expression, we get
(1 KJ = 1000 J)
Therefore, the enthalpy change for converting 1 mole of ice at to water at
is, 7.712 KJ