A pot containing 500 g of water at 100 degrees Celsius would require how much energy to boil off completely
To calculate the amount of energy required to boil off water, you can use the specific heat capacity and the latent heat of vaporization of water. Here are the steps to determine the energy needed:
1. Determine the specific heat capacity of water: The specific heat capacity of water is 4.186 J/g°C. This means that it takes 4.186 joules of energy to raise the temperature of 1 gram of water by 1 degree Celsius.
2. Calculate the energy needed to heat the water to its boiling point: Since the water is initially at 100 degrees Celsius, the temperature needs to be raised by 100 degrees Celsius to reach its boiling point. Therefore, the energy required to heat the water is:
Energy = specific heat capacity * mass of water * temperature change
= 4.186 J/g°C * 500 g * 100 °C
= 209,300 J
3. Calculate the latent heat of vaporization of water: The latent heat of vaporization of water is the amount of energy required to change 1 gram of water from a liquid state to a gaseous state at its boiling point. For water, this value is approximately 2,260 J/g.
4. Calculate the energy needed to boil off the water: Since the entire 500 grams of water needs to be boiled off, multiply the mass of water by the latent heat of vaporization:
Energy = latent heat of vaporization * mass of water
= 2,260 J/g * 500 g
= 1,130,000 J
5. Calculate the total energy needed: To find the total energy required to boil off the water, add the energy needed to heat the water to the energy needed to vaporize it:
Total Energy = Energy to heat + Energy to vaporize
= 209,300 J + 1,130,000 J
= 1,339,300 J
Therefore, it would require approximately 1,339,300 joules of energy to boil off completely a pot containing 500 grams of water at 100 degrees Celsius.