While `1mol` of ice melts at `0^(@)C` and at constant pressure of `1atm, 1440 cal` of heat are absorbed by the system. The molar volume of ice and water are `0.0196` and `0.0180L` respectively. Calculate `DeltaH` and `DeltaU`.

Explanation

To calculate the change in enthalpy (ΔH) and the change in internal energy (ΔU) for the melting of ice, we can follow these steps:

### Step 1: Understand the process
When 1 mole of ice melts at 0°C and 1 atm, it absorbs 1440 calories of heat. This heat is the enthalpy change (ΔH) for the melting process.

### Step 2: Calculate ΔH
Since the problem states that 1440 cal of heat is absorbed during the melting of ice, we can directly assign this value to ΔH:
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