Lesson: Heat of VaporizationPhysics
In this lesson, we will learn how to relate the mass conversion between liquid and gas states to net heating and the latent heat of vaporization.
Sample Question Videos
On a certain dry sunny day, a swimming pool’s temperature would rise by if the water in the pool did not lose some internal energy by evaporation. Determine the percent of the water in the pool that must evaporate to remove precisely enough internal energy to keep the water temperature constant. Use a value of for the specific heat capacity of water and use a value of 2,430 kJ/kg for the latent heat of vaporization of water.
A man consumes 3,000 kcal of food in one day, converting most of it to thermal energy to maintain body temperature. If he loses half this energy by evaporating water (through breathing and sweating), how many kilograms of water evaporate?
For specific latent heat of vaporization of water, use 2,430 kJ/kg.
Indigenous people sometimes cook in watertight baskets by placing hot rocks into water to bring it to a boil. What mass of granite must be placed in 4.00 kg of water to bring its temperature to if 0.0250 kg of water escapes as vapor from the initial sizzle? Take the specific heat capacity of water to be , the specific heat capacity of granite to be , and the specific latent heat of vaporization of water to be 2,256 kJ/kg. You may neglect the effects of the surroundings.