If you assume that the density of sweat is the same as that of water (1g/ml) and that the specific heat of sweat is the same as that of water (4.184 J/g/deg), then one can estimate the heat required to evaporate 7.24 ml of sweat at 25 degrees Cheat to raise 7.24 ml from 25º to 100º = q = mC∆T = (7.24g)(4.184 J/g/deg)(75deg) = 2272 J
heat to evaporate 7.24 ml = q = m∆Hvap = (7.24g)(2260 J/g) = 16,362 J
Total heat = 2272 J + 16,362 J = 18,634 J = 18.6 kJ
Heat of vaporization
The energy needed to completely vaporize a mole of a liquid
The answer is 55,117 kJ.
The boiling point of ethanol is 78 C but it can evaporate slowly at just room temperature. You can set it on fire and it will vaporize even more quickly.
The amount of energy required to turn a more of a liquid into a gas - apex
cotton allows sweat to vaporize and it absorbs heat.
Gasoline has a less boiling point (72 degree Celsius) While water has a bigger boiling point (100 degree Celsius)
Heat of vaporization
The energy needed to completely vaporize a mole of a liquid
The amount of time depends on the latent heat of vaporisation and the latent heat of melting.
The answer is 55,117 kJ.
1oo calories for 1 g
The boiling point of ethanol is 78 C but it can evaporate slowly at just room temperature. You can set it on fire and it will vaporize even more quickly.
you sweat to stay cool. The heat of the sun is used to turn your sweat to water vapor, rather than to heat up your body.
No, when you sweat the sweat evaporates and takes the heat away
If it is close enough to the burst, nothing. The million degree plus thermal flash will simply vaporize it!
Humans sweat in a tropical heat.