Determine the value of `DeltaH` and `DeltaU` for the reversible isothermal evaporation of `90.0g` of water at `100^(@)C`. Assume that water behaves as an ideal gas and heat of evaporation of water is `540 cal g^(-1) (R = 2.0 cal mol^(-1)K^(-1))`.

Explanation

To determine the values of ΔH (enthalpy change) and ΔU (internal energy change) for the reversible isothermal evaporation of 90.0 g of water at 100°C, we can follow these steps:

### Step 1: Calculate the number of moles of water
The molecular weight of water (H₂O) is approximately 18 g/mol.

\[ \text{Number of moles} = \frac{\text{mass of water}}{\text{molecular weight}} = \frac{90.0 \, \text{g}}{18 \, \text{g/mol}} = 5 \, \text{moles} \]
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