The freezing of water at 0⁰C can be represented as follows:

H2O (l) ↔ H2O(s)
The density of liquid water is 1.00 g/cm3. The density of ice is 0.92 g/cm3. explain why applying pressure causes ice to melt.

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The volume of solid H2O (ice) is higher than the volume of the liquid. Applying pressure will cause the reaction shown to shift to the side that occupies the lower volume. That is the liquid side so the solid melts.

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I have a source but not allowed to post internet url's :(

copy and paste it ? Im gonna have to make it into my own words anyway

If you can't its okay :)

When pressure is applied to a substance, it affects the arrangement of its molecules or atoms. In the case of ice, which is the solid phase of water, applying pressure can cause the ice to melt and become liquid water. This may seem counterintuitive, as we generally think of applying pressure as causing things to solidify rather than melt.

To understand why pressure causes ice to melt, we need to consider the differences in molecular arrangement between the solid and liquid phases of water. In the solid state, the water molecules in ice are arranged in a regular, lattice-like structure held together by hydrogen bonds. These hydrogen bonds give ice its unique crystal structure.

When pressure is applied to the ice, it compresses the molecular arrangement, increasing the density of the substance. This compression disturbs the hydrogen bonds and disrupts the organized lattice structure of the ice. As a result, the ice begins to melt, and the molecules gain enough mobility to transition into the less dense liquid phase.

Furthermore, the increase in pressure also raises the melting point of water. Under normal atmospheric pressure, water freezes at 0⁰C. However, when pressure is applied, the melting point of the ice increases. This happens because the increased pressure favors the formation of a more densely packed solid phase. So, applying pressure effectively raises the temperature at which ice can exist as a solid.

To summarize, applying pressure to ice disrupts the hydrogen bonds and the regular structure of the ice, allowing it to melt and transition into liquid water. The increase in pressure also raises the melting point of the ice, causing it to melt at a higher temperature than under normal atmospheric conditions.