# Can I consider this scenario for the phase change of $H_2O_{(s)}$ to $H_2O_{(L)}$

From a particular topic : Enthalpy changes during phase transformations.

It says in my textbook that standard state of a substance at a specified temperature is it’s pure form at 1 bar pressure.

Let’s consider the phase change for $$H_2O(s)$$ to $$H_2O$$ (L). $$\delta H$$ of fusion with a subscript I.e - . It’s value is 6 kJ/mol is value needed for such a change.

This phase change is happening at a standard state according to my textbook. Here . I have drawn is the image of how is the phase change happening. Mostly , I have just combined all the definition and statements.

The $$\delta H$$ of fusion is at standard state. I.e it has a pressure of 1 bar of its own and a specified temperature. It is the amount of energy needed to melt $$H_2O$$ (s).

The surrounding are at a temperature = 273K and pressure = 1 atm.

When ice melts at 273K. It is converted to water at 273K. Same temperature. Pressure in scenario is always 1 atm.

I wish to confirm my scenario. 