Answer 1) : When we calculate the ΔQ = -40.66 kJ (heat of vaporisation).
Then, we can relate the work done with this equation,
ΔW = -PΔV
First we need to calculate the volume, which will be,
Volume of water vapor = (nRT) / (P)
Then, V = (1 mole) X (0.0821 L X atm/mole X K) X (373.15K) / (1atm) = 30.6 liters So, it is given, and verified.
Volume of Water can be used for finding the; Density = M / V
D = ( 1 mole) X (18.02 g/mole) / (18.80 mL) = 0.9585 g/mL
On, substituting the values, we get,
ΔW = -PΔV
Work = - (1 atm) X (0.00188L - 30.62L) X 0.1013kJ/L X atm = 3.10 kJ
hence the work done is 3.10 kJ
Answer 2) Now, for calculating the internal energy, we can use the formula as,
ΔE = ΔQ + ΔW
Here, we have the values of ΔQ = -40.66 kJ and ΔW as = 3.10 kJ
So, we get, ΔE = (-40.66) + (3.10) = - 37.55 kJ
Therefore, the change in the internal energy will be -37.55 kJ.
