The enthalpy of fusion of ice, an endothermic process, involves calculating the heat interactions between melting ice and water in a calorimeter, demonstrating the conservation of energy.
The experiment in question involves the melting of ice at 0 degrees Celsius and determining various heat-related values such as the heat lost by water, the heat absorbed by melted ice, and the heat of fusion of ice.
Fusion (melting) is an endothermic process because it absorbs heat.
To calculate the heat lost by water in the calorimeter, the mass of the water must be multiplied by its specific heat capacity and the change in temperature.
To calculate the heat absorbed by melted ice, its mass and the temperature change would be used alongside the specific heat capacity for water.
Lastly, the heat gained by ice during the melting process can be determined using the mass of the ice and the enthalpy of fusion.
Energy transfer between the ice and water in the calorimeter illustrates the conservation of energy, where the energy lost by water is equal to the energy gained by the ice, with no net change in the entropy of the universe.
Systems interacting in the experiment: The system is the ice, and the surroundings constitute the water in the calorimeter.
The direction of energy flow is from the warmer water to the colder ice.
Energy conservation: Energy is conserved as the heat lost by the water in the calorimeter is gained by the ice, maintaining the entropy of the universe.