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How many calories are needed to vaporize 1 gram of boiling water at 100 degrees?
Datboikev3fb2910
540 calories are needed to turn one gram of water at 100 degrees celsius to steam.
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∙ 9y ago
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How many joules of heat are needed to completely vaporize 24.40 grams of water at its boiling point?
The answer is 55,117 kJ.
How much heat is needed to vaporize 1.25 kg of ethanol?
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.
What is the amount of energy needed to vaporize one gram of a liquid?
Heat of vaporization
4 kg of ice at 0 degrees Celsius is converted to steam at 100 degrees Celsius How much heat is needed?
It takes 80 calories per gram to increase the temperature of water by one degree. 4000 * 80 * 100 = 32000000 calories.
What information does the latent heat of vaporization give?
The energy needed to completely vaporize a mole of a liquid
How much heat energy is needed to vaporize g of water at its boiling point of K?
1oo calories for 1 g
How much energy will be needed to vaporize 175g of water?
The amount of energy needed to vaporize 175 g of water depends on the temperature of the water. However, we shall assume it is 100 degrees C. We multiply 175 by 539 and get 94,325 calories. (Notice the small c). We could express it as 94 Calories if we were talking about the stuff on your dining room table.
How many calories are needed to change 1 gram of 100 degrees Celsius boiling water to 100 degrees Celsius steam?
This is the latent heat of vaporisation of water, which at standard pressure, is 539 calories (per gram).
How many joules of heat are needed to completely vaporize 24.40 grams of water at its boiling point?
The answer is 55,117 kJ.
How much heat is needed to vaporize 1.25 kg of ethanol?
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.
Why is more heat needed to vaporize water than gasoline?
Gasoline has a less boiling point (72 degree Celsius) While water has a bigger boiling point (100 degree Celsius)
Why doesnt the all the water instantly vaporize when you reach the boiling point?
The boiling point is the temperature where a substance BEGINS to vaporize. So all of the water doesn't necessarily need to boil off instantly. To vaporize, molecules of water need to have energy. Only at the boiling point do they have enough energy to boil away, and when they do, they carry this energy with them. This means that a constant supply of heat for a certain period of time is needed for all water in a sample to boil off.
How many calories are needed to heat 225 g of water from 50.5 degrees C to steam at 133 degrees C?
1 cal/gdegC x 225g x (100 - 50.5)degC heat to the boiling point 540 cal/g x 225g heat to vaporize the water 0.5 cal/gdegC x 225 g x (133-100)degC heat to chang temp of steam = 11137.5 cal + 121500 cal + 3712.5 cal = 14850 cal
How many calories are needed to raise the temp of 8.1 g of water 20 degrees Celsius?
there are no calories in water you idiot
How much energy is needed to raise the temperature of 2.0 g of water 5.0 degrees C?
The needed energy is 10 calories.
What is the total number of calories of heat needed to raise to raise the temperature of the liquid water from 20 degrees Celsius to 30 degrees Celsius?
The number of calories required will depend on the mass of water which is to be heated.
What is the amount of energy needed to vaporize one gram of a liquid?
Heat of vaporization
