Conclusion question(s) from a lab we did to find the heat of fusion of ice:
Does the value obtained for the molar heat of fusion depend on the volume of water used? Does it depend on the mass of ice melted? Does it depend on the final temperature of the mixture?
The heat of fusion should be in heat units per unit mass, so it should not depend on mass. The heat of fusion is a physical charactistic of a particular compound, it does not depend on anything except what compound is being examined.
i need help in heat of fusion my mean old teacher made us do 15 pages of heat of fusion and i am only in 5 grade!!!
6000 calories of heat are added to 32g of water at 100 degree celsius. what is the resulting temperature?
in what way does calorimetry make use of law of conservation of energy?
When water is frozen into ice cubes in the freezer, where does the released heat go?
HOW DO YOU FIGURE OUT THE SPECIFIC HEAT. TO DETERMINE THE HEAT OF FUSION OF ICE
i believe calorimetry displays the law of conservation of energy because in the calorimeter, heat/energy is neither gained nor lost.
a,,,e,,,wala
no to all of the above
i am looking for the result of the experiment
how many kilojoules are released when 35.0g of water at 65.0 celcius is cooled to 0.0 celcius and changed to solid?
To determine the specific heat and heat of fusion of ice, you can use the following steps:
1. Measure the mass of the ice you are using. Let's say you have "m" grams of ice.
2. Measure the initial temperature of the ice. Let's say it is "T_initial" degrees Celsius.
3. Place the ice in a container and add a known mass of water to it. Let's say you add "M" grams of water to the ice.
4. Measure the initial temperature of the water. Let's say it is "T_water_initial" degrees Celsius.
5. Stir the mixture of ice and water and allow it to reach thermal equilibrium. This means that the ice and water are at the same temperature.
6. Measure the final temperature of the mixture once it reaches thermal equilibrium. Let's say it is "T_final" degrees Celsius.
Now, to calculate the specific heat of water and the heat of fusion of ice, you can use the following formulas and equations:
1. Calculate the heat gained by the water:
Q_water = M * specific heat of water * (T_final - T_water_initial)
The specific heat of water is typically around 4.18 J/g°C.
2. Calculate the heat lost by the ice (heat used to melt the ice):
Q_ice = m * heat of fusion of ice
The heat of fusion of ice is typically around 334 J/g.
3. Assuming that there is no heat exchanged with the surroundings (adiabatic conditions), use the conservation of energy:
Q_ice = -Q_water
This equation is based on the principle that energy is conserved in a closed system.
4. Rearrange the equation to solve for the heat of fusion of ice:
heat of fusion of ice = (M * specific heat of water * (T_final - T_water_initial)) / m
Note that in order to obtain accurate results, it is important to use precise measurements and ensure good thermal contact between the ice and water.
I hope this helps! Let me know if you have any further questions.