Calculate the mass of water that can be vaporized with 211 kJ of heat at the boiling point.

Chemistry by OpenStax (2015-05-04)
1st Edition
ISBN:9781938168390
Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Publisher:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Chapter10: Liquids And Solids
Section: Chapter Questions
Problem 44E: The enthalpy of vaporization of water is larger than its enthalpy of fusion. Explain why.
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Calculate the mass of water that can be vaporized with 211 kJ of heat at the boiling point.

Expert Solution
Step 1

Heat of water (q) = 211 KJ

Mass of water (m) = ?

• Heat is related with enthalpy of vaporization as given by formula :

q = m.∆Hvap  Or

m = q / ∆Hvap 

On multiply this value with molar mass of water, we can get mass of water. So,

m = (q / ∆Hvap ) × M

Where, 

q = heat of water ; m = mass of water.

∆Hvap = Enthalpy of vaporization of water & = 40.65 KJ/mol at 100°C (i.e boiling point)  ...(we know).

M = molar mass of water & = 18 g/mol  ...(we know).

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