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When1 mole of ice melt at 0^(@) C and at...

When1 mole of ice melt at `0^(@)` C and at constant pressure of 1 atm . 1440 calories of heat are absorbed by the system. The molar volumes of ice and water are 0.0196 and 0.0180 litres respectively. Calculate `DeltaH` and `DeltaE` for the reaction.

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To solve the problem, we will calculate the change in enthalpy (ΔH) and the change in internal energy (ΔE) for the melting of ice at 0°C and 1 atm pressure. ### Step 1: Calculate ΔH (Enthalpy Change) At constant pressure, the heat absorbed by the system is equal to the change in enthalpy (ΔH). Given that 1440 calories of heat are absorbed when 1 mole of ice melts, we can directly state: \[ \Delta H = 1440 \text{ calories} \] ...
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