Question

The ΔHfus of H2O(s) is 6.010 kJ/mol. How much energy will it take to melt 25.00 g of ice?

Answer 1

Approximately `8.35` kilojoules.

Explanation:

We got `25 \ "g"` of ice, and so let's convert it to moles of ice.

Ice is just water, and will therefore have a chemical formula of `H_2O`, and its molar mass will be `18.01528 \ "g/mol"`.

So here, there exist:

`(25color(red)cancelcolor(black)"g")/(18.01528color(red)cancelcolor(black)"g""/mol")~~1.39 \ "mol"`

Now, we use the latent heat formula, which states that,

`q=mL`

• `m` is the mass of substance

• `L` is the latent heat of fusion, vaporization, etc. of substance

In this case, we got:

`q_"melt"=1.39color(red)cancelcolor(black)"mol"*(6.01 \ "kJ")/(color(red)cancelcolor(black)"mol")~~8.35 \ "kJ"`