Calculate the enthalpy change, ΔH, for the process in which 14.5g of water is converted from liquid at 10.5∘C to vapor at 25.0∘C.

For water, ΔHvap = 44.0kJ/mol at 25.0∘C and Cs = 4.18 J / (g⋅∘C) for H2O (l).

You need to calculate two stages: 1) heating of liquid water from 10.5 °C to 25.0° C, and 2) vaporization of water at 25.0°C.

1) Heating of liquid water

ΔH = m*Cs*ΔT = 14.5 g * (1kg / 1000g) * 4.18 J / (kg°C) * (25.0°C - 10.5°) = 0.878845 J

2) Heating of vaporization

You need to pass the mass in grams to moles, that is why is divide by the molar mass of water, 18 g/mol.

ΔH = n * ΔH vap = [14.5g / 18 g/mol] * 44.0 J/mol = 35.44 J

3) Total enthalpy change

ΔH = 0.879 J + 35.44 J = 36.32 J

Answer: 36.32 J