41,800
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.
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).
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.
The necessary heat is 9,22 joules.
1oo calories for 1 g
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.
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.
The specific heat of water determines how much energy is needed to heat water.
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).
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.
The needed heat is 2 258 kJ.
It depends on how much it needs to be cooled down, or transferred. The more heat there is the more coolant (water) is needed.
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.
The necessary heat is 9,22 joules.
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.
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.
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.