Question: In typical ice, there are four hydrogen bonds per H₂0 molecule, each with bond strength ~0.17 eV. Surprisingly, there are also approximately four hydrogen bonds per H₂0 molecule in cold water.

1. As water freezes into ice, some additional hydrogen bonds are formed. Is the formation of these bonds an endothermic or exothermic process? Explain briefly.

2. Experimentally, 334 J of energy is required to melt 1 g of ice. Assuming that this energy goes into breaking hydrogen bonds, what fraction of the hydrogen bonds break as the ice melts? You may assume the temperature is fixed at T = 0 C as the ice melts.