Compare the amount of heat required to vaporize a 200.-gram sample of H2O(ℓ) at its boiling point to the amount of heat required

Question

Ksju [112]

3 years ago

5

Compare the amount of heat required to vaporize a 200.-gram sample of H2O(ℓ) at its boiling point to the amount of heat required

to melt a 200.-gram sample of H2O(s) at its melting point.

Chemistry

1 answer:

stira [4] · Answer 1 · 2022-04-03T12:33:17+03:00

stira [4]3 years ago

6 0

The enthalpy of vaporization of H2O is higher than the enthalpy of fusion of H2O, therefore vaporizing the same mass of H2O would require more heat/energy than melting the same mass of H2O.