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First you need to know at what temp. is the ice?

The latent heat of fusion for ice at 32 degrees F is 144 but per pound.

This will change 1 pound of ice at 32 degrees F into water at 32 degrees F.
It is defined as the amount of heat required for the 1 mole of ice to bring a change in its state, that is, from solid state to liquid state. It is also known as enthalpy of fusion, specific melting point or latent heat of fusion of ice. The particular temperature at which there is a change in the state of the ice is known as the melting point of ice.

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The amount of heat necessary to change 1 kg of a solid into a liquid at the same temperature is called the?

molar heat of fusion


The molar heats of sublimation and fusion of iodine are 62.3kjmol and 15.3kjmol respectively calculate the molar heat of vaporization of liquid iodide?

It is a known fact : Molar heat of sublimation = molar heat of fusion + molar heat of vaporization so, molar heat of vaporization = molar heat of sublimation - molar heat of fusion Mv = 62.3 kJ/mol - 15.3 kJ/mol Mv = 47 kJ/mol.


How much heat in kJ is required to melt 54.0 g of ice at 0 and degC into water at 0 and degC if and DeltaHfus for water 6.01 kJmol?

The first step is to convert the mass of ice to moles using the molar mass of water (18.015 g/mol). Then, use the molar enthalpy of fusion to determine the heat required to melt the ice. Finally, multiply the molar enthalpy of fusion by the number of moles of water to get the total heat required in kJ.


What is the molar heat of fusion of water?

The specific latent heat of fusion of water is 334 kJ/kg. Ice melts at 0 degrees Celsius and boils at 100 degrees Celsius.


How does molar enthalpy of fussion of ice compare with the molar enthalpy of fussion of other solids?

The molar enthalpy of fusion of ice is relatively high compared to the molar enthalpy of fusion of many other solids. This is because ice requires a significant amount of energy to change from a solid to a liquid state due to its strong hydrogen bonds. However, there are some solids, such as metals, that have higher molar enthalpies of fusion than ice.


What is the relation of the molar heat of fusion to the molar heat of vaporization?

Molar heat of fusion: the heat (enthalpy, energy) needed to transform a solid in liquid (expressed in kJ/mol). Molar heat of vaporization: the heat (enthalpy, energy) needed to transform a liquid in gas (expressed in kJ/mol).


How do you calculate the molar heat of fusion?

Use Einstein's Theory of Special Relativity


How are the heat of fusion of ice and heat of fusion of water similar?

due to the anomalous behaviour of water.....


What do you need to know to calculate the heat needed to melt a block of ice at its melting point?

To calculate the heat needed to melt a block of ice at its melting point, you need to know the mass of the ice block, the specific heat capacity of ice, and the heat of fusion of ice (or latent heat of fusion). The formula to calculate this heat is Q = m * ΔHf, where Q is the heat energy, m is the mass, and ΔHf is the heat of fusion.


A sentence for heat of fusion?

Because of the heat of fusion the ice is now water


What is the molar heat of fusion of ethanol?

The molar heat of fusion of ethanol is approximately 5.02 kJ/mol. This is the amount of energy required to convert one mole of solid ethanol into liquid ethanol at its melting point of -114.1°C.


What is the scientific name for ice forming and melting?

For forming it is Heat of (Fusion) and for melting its Heat of (Vaporization).