As a domain expert in thermodynamics, I am well-versed in the concepts of entropy and its implications in various physical processes. Entropy, often denoted by the symbol 'S', is a fundamental concept in the second law of thermodynamics, which describes the degree of randomness or disorder in a system. It is a state function and is measured in units of joules per kelvin (J/K).

When we discuss the entropy of water, we are typically referring to the entropy change that occurs during a phase transition, such as the transition from solid (ice) to liquid (water). The entropy change associated with this process is a measure of the increase in disorder as the ice melts and the molecules move more freely in the liquid state compared to the rigid structure of the solid state.

The entropy change for a phase transition can be calculated using the formula:

\[ \Delta S = \frac{Q}{T} \]

Where:
- \( \Delta S \) is the entropy change,
- \( Q \) is the heat absorbed or released during the phase transition (in joules),
- \( T \) is the temperature at which the transition occurs (in kelvin).

For water, the phase transition we are most interested in is the melting of ice at 0 degrees Celsius (or 273.15 K). The enthalpy of fusion for water, which is the amount of heat required to convert one gram of ice at its melting point to liquid water without changing the temperature, is approximately 333.55 J/g. Using this value, we can calculate the entropy change for the melting of ice:

\[ \Delta S = \frac{-Q}{T} = \frac{-333.55 \, \text{J/g}}{273.15 \, \text{K}} \]

The negative sign indicates that the entropy of the system increases as the ice melts, which is consistent with the increase in disorder.

Now, let's proceed to the next steps as per your instructions.

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The entropy of the system, which is --QT, increases by --Q273 K. The heat --Q for this process is the energy required to change water from the solid state to the liquid state, and is called the enthalpy of fusion, i.e. --H for ice fusion.read more >>