The system consists of 1.8 g of H2O in a diathermic cylinder sealed from the out

Question

The system consists of 1.8 g of H2O in a diathermic cylinder sealed from the outside by a freely movable massless piston. In the initial state, the system is completely in the liquid phase, H2O (l), at 100.oC and 1.00 atm and is in equilibrium with the surroundings. In the final state, as a result of heating the cylinder, the system is completely in the vapor phase, H2O (g), at 100.oC and 1.00 atm.

Calculate the expansion work, w, associated with the complete vaporization process of 1.8 g of water liquid at 100.oC and 1.00 atm. In this question, you will neglect the initial volume of 1.8 g of water liquid at 100.oC and 1.00 atm in your calculations. To calculate the volume of vapor, you can again assume that water vapor behaves as an ideal gas.

Explanation / Answer

Convert the initial 1.8 g of water into its volume using the density equation.

water Density: 999.97 kg/m³ so the volume = 0.0018/999.97 = 1.8*10-6 m3

w=PdV

= 1*1.8*10-6 = 1.8*10-6 atm-m3

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