Calculate the latent heat of fusion of ice. 1.The inner cup of the calorimeter and the stirrer was weighed using a triple balance. The mass of 50.0g was recorded 2. The inner calorimeter cup was filled about ¾ full of water with an initial temperature of 45°C. 3. The total mass of the cup with water of 158.0g was measured. 4. Find the mass of the water. 5. A mass of ice cube at 0°C was poured into the calorimeter cup with water. The system was insulated by the outer calorimeter cup. This was covered and stirred. The final temperature of 33°C was read upon equilibrium temperature was reached. 6. The total mass of the cup, stirrer, water, and ice of 170g. 7. Find the mass of the ice cubes. 8. Using the law of conservation of energy or
Latent heat and phase change
A physical process in which a conversion among the basic states or phases of matter, i.e., solid, liquid, and gas takes place under the effect of a certain temperature and pressure is referred to as a phase change. Generally, the phase change of a substance occurs when heat transfer takes place between the substance and its surroundings. Based on the direction in which heat transfer takes place, different types of phase changes can occur.
Triple Point of Water
The branch of physics in which observer deals with temperature related properties is called thermodynamics.
Boiling Point of Water
Everyday examples of boiling is, boiling milk, heating water. One would have observed that when we heat water it goes through various stages and at one point bubbles show in water, and water keeps splashing with bubbles bursting, we in layman terms say that water is boiling.
Freezing Point of Water
In general, the freezing point of water is 0° Celsius, or 32° Fahrenheit. This is the temperature at which water will ordinarily change from its liquid state to its solid state (ice). However, there are certain conditions that can affect the freezing point of water. For example, a liquid may be supercooled or contain impurities so that it does not freeze at the ordinary freezing point.
Calculate the latent heat of fusion of ice.
1.The inner cup of the calorimeter and the stirrer was weighed using a triple balance. The mass
of 50.0g was recorded
2. The inner calorimeter cup was filled about ¾ full of water with an initial temperature of 45°C.
3. The total mass of the cup with water of 158.0g was measured.
4. Find the mass of the water.
5. A mass of ice cube at 0°C was poured into the calorimeter cup with water. The system was
insulated by the outer calorimeter cup. This was covered and stirred. The final temperature
of 33°C was read upon equilibrium temperature was reached.
6. The total mass of the cup, stirrer, water, and ice of 170g.
7. Find the mass of the ice cubes.
8. Using the law of conservation of energy or the method of mixture, find the experimental
value EV of the latent heat of fusion of ice Lf. The calorimeter cup and the stirrer are
made of aluminum.
Q gained + Q Lost = 0
mC ΔTcold substance + m C ΔTwarm substance = 0
miLf + miCw ΔT (melted ice ) + mC ΔT (cup) + mC ΔT (water) = 0
For the cold substance and based from the graph of phase changes, start with Q2 = miLf because
the ice is at 0°C, then Q3 = miCw (T2 – T1); where: mi is the mass of the ice, Cw is the specific
heat of water, Ti = 0°C while T2 is he final temperature of the mixture.
For the warm substances, the heat is released from the cup and water, thus they have common
ΔT= T2 – T1 where: T1 is the initial temperature of the water and cup, while T2 is he final
temperature of the mixture.
9. Solve for the percentage error using the True Value TV of Lf = 80 cal/g°C
10. Compete the data table.
Data Table
Mass of the inner cup and stirrer, mc (g)
Total mass of the cup, stirrer and water (g)
Mass of the water, mw (g)
Initial temperature of the cup and water, T1 (°C)
Total mass of the cup, water and ice
Mass of the ice mi (g)
Initial temperature of the ice T1 (°C)
Final temperature of the mixture T2 (°C)
Experimental value of the Latent heat of Fusion, EV of Lf (cal/g°C)
True Value of the Latent Heat of Fusion, TV of Lf (cal/g°C)
% error
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