2.5 g 1 mol/18.02 g (-285.83) kJ/mol
How much water, and what temperature is it, and what temperature is the ice? Also, what temperature are the surroundings?
It's possible in theory to answer this question, but you haven't given us enough details.
In actual practice, you probably cannot freeze water using nothing but ice.
it takes 1589kj to freeze water that is at 15 degrees Celsius
Freezing is the act of removing energy from something but if you're using a freezer then yes, because the freezer needs energy to operate.
how much energy is generated from freezing 2.5 g water?
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2.5g x 1mol/18.02 g x (6.03) kj/mol
0
2.5 g 1 mol/18.02 g (-285.83) kJ/mol
2.5 g 1 mol/18.02 g (-285.83) kJ/mol
Other comment is wrong 2.5 g 1 mol/18.02 g (-285.83) kJ/mol
A lot
0
2.5 g 1 mol/18.02 g (-285.83) kJ/mol
You need to know the initial temperature.
2.5 g 1 mol/18.02 g (-285.83) kJ/mol
Other comment is wrong 2.5 g 1 mol/18.02 g (-285.83) kJ/mol
A lot
None. When water freezes it _releases_ energy (the heat of fusion, 333.55 kj.kg). To keep it from freezing, simply keep the energy constant. If the ambient temperature is below zero C (32 F) the rate of energy loss will depend on the temperature of the air and the thermal resistance (insulation value) of the water's container, and other factors such as wind speed. In those conditions you must replace the energy lost to prevent the water from freezing. However, the energy needed depends on the rate of loss, not on the amount of water.
No heat (energy) is required to freeze water (from liquid to solid). Freezing RELEASES energy (heat), as it is an exothermic event. If you want to know how much energy is release, you need to know the heat of fusion for water, and then multiply that by the mass of water being frozen.
Air compressor alone consumes about 50 to 60 % of energy generated by a gas turbine..
2.5 g 1 mol/18.02 g (-285.83) kJ/mol
Realistically none of the worlds energy needs are done in this manner.
It depends on how much sugar is in the water.