ACTIVITIES 京 Activity 1. Directions: Carefully read the following statements below, write TRUE if the statement is correct, FALSE if it is not.
1. Universe is composed of system and surroundings.
2. The heat that is released by the surroundings should be absorbed by the system.
3. In a chemical reaction, energy is lost in the form of heat
4. The "Cal” present on the label of food products is equal to 4.184 J
5. Work is the transfer of thermal energy between two bodies that are at different temperatures.
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The heat required to vaporize the water is 76.266 kJ or 76266.32 J.
Explanation:Heat of Vaporization
Vaporization or commonly known as evaporation is the process where the liquid generates a vapor pressure above itself.
The heat of vaporization or the enthalpy of vaporization (ΔH vap) is the heat required in order to change the phase of the liquid.
The molecules of a liquid moves constantly and have a various range of kinetic energies. There will be a time that some of the liquid's molecules will have enough energy to escape from the surface and eventually will enter the gas phase (vapor phase).
For this problem, we can use the known enthalpy of vaporization of water.
The enthalpy of vaporization of water is 2256.4 J/g. This means that in order to convert 1 g of water at 100°C to steam at 100°C, a heat amounting to 2256.4 J is required.
For our case, we have a mass of water amounting to 33.8 g at 100°C and we want to vaporize it to steam (also at 100°C).ΔH vap = 2256.4 J/g * 33.8 gΔH vap = 76266.32 J = 76.266 kJ
Therefore, the heat required to vaporize the water is 76.266 kJ or 76266.32 J
Learn more about heat of vaporization here:
More example problems of vaporization/ evaporation here:
Distillation tower uses the technique of fractional distillation to seperate its components from crude oil.
Fractional distillation exploits the difference in boiling point of the components to seperate it.
Boiling point is the answer.