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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 heat is needed to convert 38.5 g of ice at 0 C to a liquid at 55 C?
To convert ice at 0°C to liquid water at 0°C, 334 J/g of heat is needed (heat of fusion). To raise the temperature of liquid water from 0°C to 55°C, 4.18 J/g°C is required (specific heat capacity of water). The total heat required would be (mass of ice x 334 J) + (mass of ice x 4.18 J/g°C x temperature difference).
How much heat is needed to freeze 100 g of water?
The heat needed to freeze 100 g of water is 334 J/g. So, for 100 g, the total heat needed would be 334 J/g * 100 g = 33,400 J.
How much energy is needed to melt 0.25 moles of water?
The necessary heat is 9,22 joules.
How much heat energy is needed to vaporize g of water at its boiling point of K?
1oo calories for 1 g
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 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.
Why does water take so long to warm up?
The specific heat of water determines how much energy is needed to heat water.
How much heat is needed to convert 38.5 g of ice at 0 C to a liquid at 55 C?
To convert ice at 0°C to liquid water at 0°C, 334 J/g of heat is needed (heat of fusion). To raise the temperature of liquid water from 0°C to 55°C, 4.18 J/g°C is required (specific heat capacity of water). The total heat required would be (mass of ice x 334 J) + (mass of ice x 4.18 J/g°C x temperature difference).
How much heat energy is needed to convert 50 kg of water at 8 degrees Celsius to steam at 100 degrees Celsius?
The process involves increasing the temperature of water from 8°C to 100°C and then changing its phase to steam at 100°C. The total heat energy required can be calculated using the specific heat capacity of water and the heat of vaporization. The formula Q = mcΔT can be used to find the heat energy needed, where Q is the heat energy, m is the mass of water, c is the specific heat capacity of water, and ΔT is the temperature change.
How much heat requires one litre of water evaporates?
The needed heat is 2 258 kJ.
How much coolant aka water is needed for a nuclear power station?
It depends on how much it needs to be cooled down, or transferred. The more heat there is the more coolant (water) is needed.
How much heat is needed to freeze 100 g of water?
The heat needed to freeze 100 g of water is 334 J/g. So, for 100 g, the total heat needed would be 334 J/g * 100 g = 33,400 J.
How much energy is needed to melt 0.25 moles of water?
The necessary heat is 9,22 joules.
How much heat is needed to raise 8 kg of water from 4 degrees Celsius to 83 degrees Celsius?
The heat needed can be calculated using the formula: Q = mc∆T, where Q is the heat, m is the mass of water, c is the specific heat capacity of water (4186 J/kg°C), and ∆T is the change in temperature. Plug in the values to find the heat needed.
How much heat is in fresh water?
It would depend on the temperature of the water, or average kinetic energy. (KE) However, what you may be looking for is how much heat is needed to raise the KE, or temperature, of water. 4.184 kilojoules per gram is the heat required to raise the temperature of water 1 degree Celsius.
How much heat is requires to convert 0.3 kilogram of ice at 0 C to water at the same temperature?
The molar heat of fusion of water in J / g is 334. To find the heat required to convert 0.3 kg, use the equation: heat of fusion * mass = heat required. It would require 100.2 kJ.
