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How much energy would be required to vaporize 28 grams of water?
Wiki User
∙ 12y ago
At standard pressure a gram of water at 100 degrees C requires 550 calories to convert it into steam at 100 degrees C.
Therefore, 234.5 grams requires 128975 calories, or 541700 Joules.
Wiki User
∙ 9y ago
Wiki User
∙ 9y agoThe original water temperature and pressure need be known to answer the question.
Wiki User
∙ 8y agoThe heat (enthalpy) of vaporization has different values for each material.
Wiki User
∙ 12y ago63280 Joules
Wiki User
∙ 11y agoapprox. 2,8 kcal (from O 0C to 100 0C)
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How much energy is gained by 3 grams of ice when it changes to water?
No energy is gained. On the contrary, energy is required to make ice melt.
What Is a source of energy that utilizes uranium-235 in a fission reaction to vaporize water The steam is then used to turn turbines to generate electricity?
nuclear power
What is Water absorption coefficient formula?
If the water is not already at boiling temperature, then you will need equations 1 and 2. If the water is already at boiling temperature, you will only need equation 2.1. Q = m X C X ΔTThis equation is used to calculate how much energy is required to change the temperature of a given object, of given mass, by a given number of degrees.Q = the total amount of energy required, in joulesm = mass, in grams, of the object being heated (in this case, the water)C = the specific heat of the object (for water, 4.186)ΔT = the total change in temperature2. Q = 2.257 joules X mThe 2.257 in this equation is the heat of vaporization of water: that is, the amount of energy, required per gram of water, to boil water: 2.257 joules per gram. If you were using this equation for a different substance, you would have to look up its heat of vaporization, and substitute it in this equation.Q = the amount of energy required, in joulesm = mass, in grams, of the waterFor example, suppose you were asked to calculate how much energy it would take to boil 256 grams of water which is currently at 40 degrees Celsius. We know that the boiling temperature of water is 100 degrees Celsius; therefore the change in temperature, ΔT, is 100 - 40, which equals 60. Calculate as follows:Q = 256 grams X 4.186 X 60°CQ = 64296.96 joulesThis is how much energy it will take to raise the temperature of the water from 40°C to 100°C. Now calculate how much energy it will take to boil the water once it reaches 100°C:Q = 2.257 joules X 256 gramsQ = 577.792 joulesWe now take the energy required to raise the temperature of the water from 40°C to 100°C and add it to the energy required to boil the water:64296.96 joules + 577.792 joules = 64874.752 joulesConvert to kilojoules:64875.752 joules / 1000 = 64.875752 kilojoulesRound to 64.88 kilojoules.If you are required to express your answer in scientific notation, then express it as6.488 x 103 kilojoules.
How much energy is required to raise 21kg of water by 2 degrees Celsius?
21 Kg = 2100 grams to rise the temperature of this amount of water by 2 degrees Celsius you need 2*2100 = 4200 calories or 17572.8 Joules.
How do you get the energy released when 150 grams of water freezes?
You need to get the energy OUT of the water; otherwise it won't freeze. This is usually done by putting the water in contact with something colder.
How much energy is gained by 3 grams of ice when it changes to water?
No energy is gained. On the contrary, energy is required to make ice melt.
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 does evaporation involve the storage of heat?
When the energy is required to vaporize liquid water, the molecules are highly agitated and brake free to become vapor through the state of latent heat of vaporization, then the energy is removed from the liquid and the temperature is reduced.
Describe the water cycle and the importance of the suns radiant energy in that cycle?
it allows the water cycle to continuously vaporize the water into mist
If the heat of fusion of water is 3.4 102 J g the amount of heat energy required to change 15.0 grams of ice at 0C to 15.0 grams of water at 0C is what?
1200 cal
What is the thermal energy needed to completely vaporize 18.02g of water at 100 degrees?
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
In order to get liquid water to become water to become water vapor what must be energy?
Energy must be added to liquid water so that it reaches the boiling point, at which point the water will vaporize into water vapor.
How much heat energy is needed to vaporize g of water at its boiling point of K?
1oo calories for 1 g
Most methods of large scale desalinization are not cost effective because?
too much energy is needed to vaporize water
How much energy is required to vaporize 2kg of water at 100c?
The latent heat for water to steam is 550 calories (2310 Joules) per gram. For 2 grammes, double these figures.
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 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.
