0
The heat of fusion for water is 6.02 kJ/mol. So we need to convert 1 gram of water into moles of water: 1 g H2O x 1 mol H2O/18.02 g H2O = 0.055 moles H2O Now we can find the heat released from freezing those 0.055 moles: 0.055 moles H2O x 6.02 kJ/1 mol H2O = 0.334 kJ of heat released Of course if we use the proper number of significant figures (since you only wrote 1g) it would be 0.3 kJ of heat released.
Wiki User
∙ 15y ago
Wiki User
∙ 14y agoHowever much you but into the water. Or, however much difference there is between the water and its environment. For example, if you have a cup of water of 25*C and the ambient temperature is 15*C, the water give out 10*C of energy. I'll let you work out the actual number in J
Wiki User
∙ 11y agoThe heat of evaporation of 1 gram of water at 100C at atmospheric pressure is 538.5 calories.
1 gram of water condensing from a 100% quality of saturation (dry steam) at 100C and atmospheric pressure releases 538.5 calories.
For lower quality the enthalpy is lower. Such that the latent heat of evaporation is reduced by the amount of moisture in the steam.
Wiki User
∙ 14y agoEnthalpy of fusion is the energy it takes to change from a solid to a liquid state (melt ice at 0°C to water at 0°C)
Wiki User
∙ 14y agoThat's called heat of fusion. Going from a liquid to a gas is heat of vaporization.
Wiki User
∙ 8y agoThisa is enthalpy of fusion and is different for each substance.
Wiki User
∙ 8y agoIt is the latent heat of melting (liquefaction).
Wiki User
∙ 13y agoless than 1 degrees Celsius
Add your answer:
Earn +20 pts
How much water is requried to condense per ton of steam?
50 times of steam
What properties of water protects organism from overheating?
water has a high heat of vapourization.it absorbs much heat as it changes from liquid to gas.it has the capacity of absorbing heat with minimum of change in its own temperature
In which temperature water has maximum specific heat capacity?
The specific heat capacity of water does not change much within-phase (ie, as a solid it has one specific heat capacity, as a liquid/gas it has another)
Why does water not heat up or cool off as air?
because the specific heat of water is very high
How much heat must be transferred to liquid water to change the waters temperature from 27 degrees Celsius to 32 degrees Celsius?
To change the temperature of water from 27ºC to 32ºC will depend on the mass of water that is present. Obviously, the more water, the more heat it will take. This can be calculated as follows:q = heat = mC∆T where m is the mass of water; C is sp. heat = 4.184 J/g/deg and ∆T is 5ºC (change in temp).
How much water is requried to condense per ton of steam?
50 times of steam
If water hardness is1000ppm then how much quantity of ethylene diamine tetra acetic acid is requried to make hardness of water 30ppm?
55 Ml.
How much more heat needs to be added to water at 100 degrees centigrade in order to change it to steam?
Heat required to have such a change of state is called latent heat. If L J/kg is the latent heat per kg of water then for M kg of water we need M* L joule of heat energy
What properties of water protects organism from overheating?
water has a high heat of vapourization.it absorbs much heat as it changes from liquid to gas.it has the capacity of absorbing heat with minimum of change in its own temperature
In which temperature water has maximum specific heat capacity?
The specific heat capacity of water does not change much within-phase (ie, as a solid it has one specific heat capacity, as a liquid/gas it has another)
Is water a good conductor for heat?
Water has a high specific heat capacity (relative to metals and other conductors), making it a poor conductor of heat (takes too much energy to change the temperature).
Why does water not heat up or cool off as air?
because the specific heat of water is very high
How much heat must be transferred to liquid water to change the waters temperature from 27 degrees Celsius to 32 degrees Celsius?
To change the temperature of water from 27ºC to 32ºC will depend on the mass of water that is present. Obviously, the more water, the more heat it will take. This can be calculated as follows:q = heat = mC∆T where m is the mass of water; C is sp. heat = 4.184 J/g/deg and ∆T is 5ºC (change in temp).
What is the equation for calculating how much heat energy (calories) transferred to or from a mass of water.?
The equation is q = mC∆T where q is the heat; m is the mass of water; C is the specific heat of water (1 cal/g/deg); and ∆T is the change in temperature.
How much heat can be stored in one cubic meter of water in a heat exchanger at 25 C?
Heat stored is based on a change in temperature. If you heat the water to 75 C, then you can extract that heat when the water is cooled to 25 C again. 1 cubic meter of water is 1,000,000 grams Heat absorbed or released = specific heat capacity x mass x change in temperature. = (1 cal / g C) x (1,000,000 g) x (75 - 25)C = 50,000,000 calories lower temperature change means less heat stored.
How can the quantity of water change people's lives?
If there is too much water, people are flooded out of their homes. If there is not enough water, you have drought, and that leads to heat stroke, thirst, and hunger.
How much heat must be transferred to liquid water to change the water's temperature from 27 C to 32 C?
This heat is: 5 x 4,18 x m = 20,9 x m (in calories) where m is the mass of water.
