Answer to Question #142265 in Molecular Physics | Thermodynamics for Victor Muwadia

Question

When 3.00g of water at 100°C changes from the liquid to the gas phase at standard atmospheric pressure, its change in volume is 2.45×10−3m3. The latent heat of vaporisation of water is 2260 kJ/kg.
How much heat must be added to vaporize the water?
How much work is done by the water against the atmosphere in its expansion?
What is the change in the internal energy of the water?

Answer 1

To vaporize the water, we need to add the following amount of heat:

$$Q=m\lambda=0.003\cdot2260=6.78\text{ kJ}.$$

The work by the water against the atmosphere in its expansion is

$$W=p\Delta V=101325\cdot2.45\cdot10^{−3}=248.2\text{ J}.$$

The change in the internal energy of the water is

$$\Delta U=Q-W=6532\text{ J}.$$