Question

What amount of energy is required to melt a 10.7 g piece of ice at 0 C? The heat of fusion of ice = 333 Jg-1

Answer 1

Approx. `3.5*kJ`...........Why?

Explanation:

We perform the physical reaction........

`H_2O(s) +Deltararr H_2O(l)`; both reactants and products are at `0` `""^@C`, and thus we need only assess the energy transfer of the PHASE change........

We are given the `"heat of fusion"` of ice in `J*g^-1`....

We gots a `10.7*g` mass of ice, and so we take the product.........

`10.7*cancelgxx333*J*cancel(g^-1)xx10^-3*J*kJ^-1=??J`....

And this represents HEAT, `Delta`, put into the system.........is the sign correct?