find change in enthalpy and change in entropy when liquid water at 30¡ãc is converted to steam at 40 bar,375¡ãc.

To find the change in enthalpy (ΔH) and change in entropy (ΔS) when liquid water at 30°C is converted to steam at 40 bar and 375°C, we need to follow these steps:

1. Determine the heat energy required for heating the liquid water from 30°C to its boiling point.
- Use the specific heat capacity of liquid water, which is approximately 4.18 J/g·°C.
- Calculate the mass of water using the given information or assume a specific quantity.

2. Determine the heat energy required for converting the liquid water at its boiling point to steam at the same temperature.
- Use the enthalpy of vaporization for water, which is approximately 40.79 kJ/mol.
- Convert the mass of water to moles using the molar mass of water, which is approximately 18.015 g/mol.

3. Determine the heat energy required for heating the steam from its boiling point to 375°C.
- Use the specific heat capacity of steam, which is approximately 2.03 J/g·°C.
- Assume the mass of steam is the same as the mass of the initial liquid water.

4. Calculate the total change in enthalpy (ΔH) by summing up the heat energy required in each step.

5. Determine the change in entropy (ΔS) using the Clausius-Clapeyron equation.
- ΔS = ΔH/T, where T is the temperature in Kelvin.

It's important to note that these calculations involve certain assumptions, such as assuming constant pressure and neglecting any phase changes other than liquid to gas. The values used for specific heat capacities and enthalpy of vaporization are approximate values and may vary slightly depending on the source.