The amount of heat lost when boiling water depends on several factors, including the initial temperature of the water, the ambient temperature, the pressure, and the duration of the boiling process.
To determine the heat lost during boiling, we need to consider the energy required to raise the temperature of the water from its initial temperature to its boiling point, as well as the energy required for the phase change from liquid to vapor.
The specific heat capacity of water is approximately 4.18 Joules per gram per degree Celsius (J/g°C), which means it takes 4.18 Joules of energy to raise the temperature of 1 gram of water by 1 degree Celsius.
To calculate the heat lost during boiling, you would need to know the mass of the water being boiled, the initial temperature, and the boiling point temperature. The heat lost can be calculated using the following formula:
Heat lost = mass × specific heat capacity × (final temperature - initial temperature)
However, it's important to note that during boiling, the temperature of the water remains constant at its boiling point until all the water has converted to steam. The energy required during this phase change is called the heat of vaporization, which for water is approximately 40.7 kilojoules per mole (kJ/mol).
So, to calculate the total heat lost during the boiling process, you would need to account for both the energy required to raise the temperature of the water and the energy required for the phase change.
It's worth mentioning that some of the heat lost during boiling is also affected by the heat transfer to the surroundings, which can depend on factors such as the container used, the insulation, and the ambient temperature.