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How much energy is required to evaporate 21.6 tons of water?
The needed energy at 100 oC is 48751 MJ.
If 30.86g of H2O is frozen (from liquid to solid) how much heat energy is required?
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.
How much energy is required to melt 56g?
The energy required to melt a substance can be calculated using the formula: Energy = mass x heat of fusion. For water, the heat of fusion is 334 J/g. Therefore, the energy required to melt 56g of water would be 56g x 334 J/g = 18,704 J.
How much energy is needed to convert ice to water on the moon?
To convert ice to water on the moon, energy is needed to break the hydrogen bonds holding the water molecules together in the solid ice lattice. This process requires the input of heat energy to overcome the enthalpy of fusion of water, which is approximately 334 joules per gram.
How much energy is required to vaporize 2 kg if aluminum?
To calculate the energy required to vaporize 2 kg of aluminum, we use the heat of vaporization of aluminum, which is approximately 10,900 J/kg. Therefore, the energy required is 2 kg × 10,900 J/kg = 21,800 J, or 21.8 kJ. This is the amount of energy needed to convert 2 kg of aluminum from a liquid to a vapor at its boiling point.
How much heat energy in kilojoules is required to convert 44.0 g of ice at -18.0 C to water at 25.0 C?
7.9
How much heat is required to convert 0.3 of ice at 0 to water at the same temperature?
The heat required to convert ice at 0°C to water at 0°C is known as the latent heat of fusion. For water, this value is 334 J/g. Therefore, to convert 0.3 g of ice to water at the same temperature, the heat required is 0.3 g * 334 J/g = 100.2 Joules.
How much heat energy in megajoules is needed to convert 7 kilograms of ice at -9c to water at 0c?
To convert 7 kilograms of ice at -9°C to water at 0°C, you need to calculate the energy required for each phase change. First, calculate the energy to raise the ice temperature from -9°C to 0°C using the specific heat capacity of ice. Then, calculate the energy required to melt the ice into water using the latent heat of fusion of ice. The total energy will be the sum of these two values.
How much energy is taken to change water into a solid?
The amount of energy required to change water into a solid is called the heat of fusion. It takes 334 joules of energy to convert 1 gram of water at 0 degrees Celsius into ice at 0 degrees Celsius. This process involves breaking the hydrogen bonds between water molecules as they transition from a liquid to a solid state.
How much energy is required to evaporate 21.6 tons of water?
The needed energy at 100 oC is 48751 MJ.
If 30.86g of H2O is frozen (from liquid to solid) how much heat energy is required?
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.
How much water is required to convert 50 baume solution of caustic to 25 baume?
1 and a half times
What versatile form do you convert much energy?
I can convert various forms of energy into electrical energy.
How much energy of is required to vaporize 1.5 kg of aluminum?
1650kj
How much energy is used make Ice?
80 cal/gram of heat is required to be extracted from water at 0 degree temp. to convert into ice at 0 degree temp.
How much energy is required to melt 56g?
The energy required to melt a substance can be calculated using the formula: Energy = mass x heat of fusion. For water, the heat of fusion is 334 J/g. Therefore, the energy required to melt 56g of water would be 56g x 334 J/g = 18,704 J.
How much energy is needed to convert ice to water on the moon?
To convert ice to water on the moon, energy is needed to break the hydrogen bonds holding the water molecules together in the solid ice lattice. This process requires the input of heat energy to overcome the enthalpy of fusion of water, which is approximately 334 joules per gram.
