How many kj of heat are needed to completely melt 32.3 g of h2o, given that the water is at its melting point? the heat of fusion for water is 6.02 kj/mole. how many kj of heat are needed to completely melt 32.3 g of h2o, given that the water is at its melting point? the heat of fusion for water is 6.02 kj/mole. 1.79 3.35 0.557 10.8 none of the above?

fourth option, 10.8 kJ

Explanation:

The heat of fusion, also named latent heat of fusion, is the amount of heat energy required to change the state of a substance from solid to liquid (at constant pressure).

The data of the heat of fusions of the substances are reported in tables and they can be shown either per mole or per gram of substance.

In this case we have that the heat of fusion for water is reported per mole: 6.02 kJ/mole.

The formula to calculate how many kJ of heat (total heat) are needed to completely melt 32.3 g of water, given that the water is at its melting point is:

The calculations are:

        number of moles = 32.3 g / 18.015 g/mol = 1.79 mol

answer: enthalpy

explanation:

for a exothermic reaction, the energy is released i.e. the energy of the products is lower than the energy of the reactants.

= enthaply

= energy of products

= energy of reactants

as , thus comes out to be negative. negative value of enthalpy shows that the reaction is exothermic.

12 is it do you think so