To calculate the energy released when freezing 2.5 g of water, we use the heat of fusion for water, which is approximately 334 J/g. Multiplying the mass of water by the heat of fusion, we get: Energy = 2.5 g × 334 J/g = 835 J. Thus, freezing 2.5 g of water releases about 835 joules of energy.
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.
2.5 g 1 mol/18.02 g (-285.83) kJ/mol
347 J/g.K or 83 cal are released.
The amount of energy generated from freezing 2.5g of water can be calculated using the specific heat capacity of water and the heat of fusion for water. The energy released would be equal to the heat of fusion of water (334 J/g) multiplied by the mass of water (2.5g). By multiplying these values, you can determine the total energy released during the freezing process.
To calculate the energy released when freezing 2.5 g of water, we use the heat of fusion for water, which is approximately 334 J/g. Multiplying the mass of water by the heat of fusion, we get: Energy = 2.5 g × 334 J/g = 835 J. Thus, freezing 2.5 g of water releases about 835 joules of energy.
Hfus of water is 333.55 (333.55j/g)(65.8g)=21947.59J 21947.59/1000= 21.947kJ I think
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
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.
For water vapours, 286 kJ/mol.
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.
2.5 g 1 mol/18.02 g (-285.83) kJ/mol
The energy released when water is condensed from water vapor is known as the heat of condensation. This process releases about 40.7 kJ of energy per mole of water condensed. To calculate the energy released when 6.0 g of water is condensed, you would first convert grams to moles and then use the molar heat of condensation to find the total energy released.
The energy released when 6 grams of water is condensed from water vapor is equal to the heat of vaporization of water. This is approximately 2260 joules per gram. So, for 6 grams of water, the total energy released would be around 13,560 joules.