Explanation:
As we know that relation between heat energy and specific heat is as follows.
Q = [tex]m \times C \times \Delta T[/tex]
Therefore, heat available will be calculated as follows.
[tex]Q_{\text{available}} = m \times C \times \Delta T[/tex]
= [tex]200 g \times 1 cal/g^{o}C \times (25 - 0)^{o}C[/tex]
= 5000 cal
Now, calculate the heat required as follows.
[tex]Q_{\text{required}} = m \times L_{fusion}[/tex]
= [tex]100 g \times 80 cal/g[/tex]
= 8000 cal
Hence, the heat required to melt the ice is more than the heat available for the reaction. Therefore, all the ice will not melt.
Thus, we can conclude that what happens is that all the ice will not melt.
