To calculate the amount of energy require to vaporise water at 100C
You need to first find the Latent heat of Vaporisation which for water is
2260kJ/kg
So to find the amount of energy required you merely multiply the mass of the water in kg by 2260.
Density of water is more or less 1kg per litre at room temperature however at 100C it could be less
The latent heat of vaporization of water is 540 cal/g at 100 °C so it would require the addition of 54,000 calories to vaporize 100 grams of water at 100 °C.
The necessary heat is:
Q = 13 . (53-18) = 455 calories
119.8 kj
40.7 kJ
The energy needed to completely vaporize a mole of a liquid
The amount of energy required to turn a more of a liquid into a gas - apex
chemical energy in batteries to thermal energy.
1650kj
Heat of vaporization
Any addition of thermal energy to a saturated liquid will cause it to vaporize. Any subtraction of thermal energy from a saturated vapor will cause it to condense.
They melt (liquefy), freeze (solidify), vaporize, or condense.
The amount of thermal energy a substance has is proportional to its temperature
The energy needed to completely vaporize a mole of a liquid
More or less everything conducts thermal energy, but to different degrees.
Because thermal energy travels from hotter objects to colder objects.
25degres celsius has more thermal energy
Anything hotter than 0 degrees that radiates heat.
You will lose thermal energy.Heat (energy) will always flow from warmer to cooler.
Your body would gain thermal energy because thermal energy only moves from something at a higher temperature to something at a lower temperature.
No. You can only convert thermal energy to other types of energy if you have a difference of temperatures between two objects, and then you can only convert part of the thermal energy. The remainder will flow from the hotter object to the colder object.
Bathtub at 45 degrees