`1` mole of ice at `0^(@)C` and `4.6 mm Hg` pressure is converted to water vapour at a constant temperature and pressure. Find `Delta H` and `Delta E` if the latent heat of fusion of ice is `80 cal//g` and latent heat of vaporisation of liquid water at `0^(@)C` is `596 cal//g` and the volume of ice in comparison to that of water (vapour) in neglected.

Explanation

To solve the problem, we need to calculate the change in enthalpy (ΔH) and the change in internal energy (ΔE) for the conversion of 1 mole of ice at 0°C to water vapor at the same temperature and pressure.

### Step 1: Calculate ΔH

1. **Latent Heat of Fusion**: The latent heat of fusion of ice is given as 80 cal/g. Since we have 1 mole of ice, we first need to convert the mass of 1 mole of ice to grams. The molar mass of water (H₂O) is approximately 18 g/mol.
\[ \text{Mass of ice} = 18 \text{ g} \]
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