2.5 g 1 mol/18.02 g (-285.83) kJ/mol
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.
2.5 g 1 mol/18.02 g (-285.83) kJ/mol
2.5 g 1 mol/18.02 g (-285.83) kJ/mol
The amount of energy required to freeze 2.5 grams of water is approximately 4.2 kJ. This energy is used to remove the heat from the water, allowing it to change from a liquid to a solid state at 0 degrees Celsius.
Hfus of water is 333.55 (333.55j/g)(65.8g)=21947.59J 21947.59/1000= 21.947kJ I think
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.
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
Approximately 6.1% of the world's energy is generated using wind turbines.
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.
To calculate the energy generated from freezing 2.5 g of water, we use the heat of fusion (Hfusion) of water, which is 6.03 kJ/mol. First, convert the mass of water to moles: (2.5 , \text{g} \div 18.02 , \text{g/mol} \approx 0.1386 , \text{mol}). Then, multiply the number of moles by the heat of fusion: (0.1386 , \text{mol} \times 6.03 , \text{kJ/mol} \approx 0.835 , \text{kJ}). Thus, approximately 0.835 kJ of energy is released when 2.5 g of water freezes.
The amount of energy required to freeze 2.5 grams of water is approximately 4.2 kJ. This energy is used to remove the heat from the water, allowing it to change from a liquid to a solid state at 0 degrees Celsius.
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
Air compressor alone consumes about 50 to 60 % of energy generated by a gas turbine..