A 315 g sample of water is heated until it has completely melted. How much heat energy was used?

1 Answer
anor277
Jun 2, 2016

We need the latent heat of fusion of ice.

Explanation:

We want the energy involved in the phase transition:

#H_2O(s) + Delta rarr H_2O(l)#

This site lists the latent of fusion of water as #334*kJ*kg^-1#. You have been given a mass of ice to start. We assume that the water and ice (i.e. the product and the reactant) remain at #0# #""^@C#.

And thus your calculation:

#334*kJ*kg^-1xx0.315*kg# #=# #??kJ#

How would energy exchange if we measured the reverse transition, liquid water to ice?

Related questions
See all questions in Thermochemistry of Phase Changes
Impact of this question
1489 views around the world
You can reuse this answer
Creative Commons License