Question

The heat of vaporization of water at 373 K is 40.7 kJ/mol. Find q, w, E, and H for the evaporation of 479g of water at this temperature. I already found q, it's (479g/18g/mol)*40.7kJ/mol=1080kJ How do I find w, deltaE, and deltaH?

Answer 1

To find w, deltaE, and deltaH for the evaporation of water at 373 K, we need additional information on the pressure change and the change in volume.

Step-by-step explanation:

To find w (work), deltaE (change in energy), and deltaH (change in enthalpy) for the evaporation of water at 373 K, we can use the following equations:

w = -P(deltaV)

deltaE = q + w

deltaH = q

Given that you have already calculated q to be 1080 kJ, we can continue with the calculations. To find w, we need to know the pressure change and the change in volume, which are not provided in the question. Without this information, we cannot calculate w or find deltaE and deltaH.