Question

Question #b01e8

Answer 1

`"33,360 J"`

Explanation:

The idea here is that the enthalpy of fusion, `DeltaH_"fus"`, tells you the amount of energy needed to convert `"1 g"` of a given substance from solid at its melting point to liquid at its melting point.

In your case, the enthalpy of fusion of water

`DeltaH_"fus" = color(darkorange)("333.6 J")color(white)(.)color(blue)("g"^(-1)`

tells you that in order to turn `color(blue)("1 g")` of ice at its normal melting point of `0^@"C"` to liquid water at `0^@"C"`, you need to provide `color(darkorange)("333.6 J")` of heat.

This means that you will need

`100.0 color(red)(cancel(color(black)("g"))) * color(darkorange)("333.6 J")/(color(blue)(1)color(red)(cancel(color(blue)("g")))) = color(darkgreen)(ul(color(black)("33,360 J")))`

The answer is rounded to four sig figs, the number of sig figs you have for the mass of the sample.