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Equipment In this lab ice and water will be mixed in a calorimeter. It is important for chemists to be able to measure this heat.
Heat of Fusion of Ice Heat of Fusion of Ice O ye frost and cold bless the Lord.
Heat of fusion of ice lab answers. Heat of Fusion of Ice Lab Questions. Some students find their experimental heat of fusion is lower than the literature value. Give a reasonable source of experimental error that would lead to a lower than literature experimental heat of fusion.
In other words explain what source of. We are trying to determine the heat of fusion for ice and compare it to the accepted value. The heat gained by the ice depends on the mass of ice multiplied by Hfusion.
To find Hfusion the equation can be rearranged and solved. Heat gained ice mice x Hfusion Hfusion Heat gained ice row 11 mice row 5 enter in row 12 7. 2 Calculate the mass of the melted ice.
3 Given the specific heat of water 4184 Jg oC calculate the energy lost by the original water. 4 Since the heat _____ by the water the heat used to _____ the ice the heat of fusion of ice Hfus can be calculated by taking the heat. V2 170mL T1 49 C T2 0 C Mass of original volume of water.
100g Volume of water. 170mL 100mL 70mL Mass of new volume of water. 170g Change in temperature.
49 C 0 C 49 C Heat lost by original mass of water. 100g X 49 C X 418 Jg C 20482J Heat of fusion of ice. 20482J 120 170g Percent error.
334- 120 X 100 64 334 Conclusion. In conclusion this lab has taught me to use. Therefore we have the equation.
M I L F M I C W T F 0 M W c W T o T F M c c c T o T F where M I is the mass of the ice L F is the heat of fusion of. Heat of Fusion of Ice Heat of Fusion of Ice O ye frost and cold bless the Lord. Praise and exult Him above all forever.
O ye ice and snow bless the Lord. Praise and exult Him above all forever. Daniel 369-70 Introduction Ice melts when the temperature is a constant 0oC.
We may be tempted to think of ice melting as a passive process. Record all masses and temperatures Mass of water Mass of ice T of water T of the system AH. In Jg Trial 1 5029 147g 240 C 82 C Trial 2 5418 1548 231 C 89 C Trial 3 528 g 167 g 236 C 100C Average AHin Jig.
The standard heat of fusion of ice is 60 kJmol. Determine percent error in the experiment Percent error. The ice undergoes a phase change.
From solid to liquid. So it must be absorbing heat energy. The coke gets cold so it must be losing heat energy.
What energy the coke loses the ice absorbs. It seems like this should be a straightforward accounting process. Subtract energy from the coke add it to the ice.
But we also need to consider what. CHEMISTRY LAB HEAT OF FUSION OF ICE INTRODUCTION. The amount of energy required to convert a solid to a liquid at constant pressure and temperature is called the heat of fusion of the substance.
In this experiment the heat of fusion of ice will be determined. The heat fusion of ice is 601 Jmol but the experimental value yielded 59 Jmol. The experiment shows that the heat fusion of ice is equal to the amount of heat needed to melt ice.
The accepted value for the heat of fusion of ice is 334 Jg. Percent Error 439 - 334 x 100 334 314. Some heat is lost to the environment because the calorimeter is not a perfect insulator.
According to this experiment the heat of fusion of ice is 439 Jg. Record all masses and temperatures. Trial 1 Trial 2 Trial 3 Mass of water 502 5413 Mass of ice 1545 1679 T of water 240C 231 C 236 C T of the system 82C 89C 100C AHin 5283 1478 Average AH in Jig.
Average AH in kJmol. The standard heat of fusion of. In this lab the ice will be melting and our goal is to find the latent heat of fusion for water L f.
The accepted value for the latent heat of fusion is 335 Jg so your calculations will hopefully be close to this value. Equipment In this lab ice and water will be mixed in a calorimeter. A calorimeter is a thermally insulating container that reduces energy transfer to the surroundings.
The calorimeter in this lab is a. Heat of Fusion of Ice Date. According to the kinetic-molecular theory all molecules are in constant random motion.
If energy is absorbed by a particle its molecular velocity will increase. Temperature is a measure of the average kinetic energy or the amount of heat per particle of a substance. Heat of fusion d.
Specific heat 3 Is the proc s of melting exothermic or endothermic. Give evidence to support 4. Draw energy diagram resent the melting of your ice.
A solid substance with a mass of 200 g is at its melting point temperature in a calorimeter While the substance changes from a solid to a. Heat of Fusion of Ice CALORIMETRY. Heat of Fusion of Ice Pre-Lab Discussion When a chemical or physical change takes place heat is either given off or absorbed.
That is the change is either exothermic or endothermic. It is important for chemists to be able to measure this heat. Heat needed to melt ice Heat needed to warm the water which was once ice M wCw T w - T f M ice Cw T f - 0 M ice Lf Eq.
Latent Heat of Fusion of ice Lf _____ calg 11. Accepted value for the Latent Heat of Fusion of ice 800 calg 12. Percent error _____ Common Errors 1.
It is important to stir the water and ice mixture to ensure that the. Using the change in temperature and the volume of ice that melts students will calculate the specific heat of ice water. Students will complete a set of calculations analysis questions and practice problems.
This lab reinforces the concepts of heat of fusion melting phase changes and endothermicexothermic reactions. Specific Heats and Calorimetry. Specific Heat of a Metal Lab.
Lab Quiz or Quiz as Exit Ticket Heating Cooling Curve of Water. Group Work Heating Cooling Curve Problems Class Summarize Heat of Fusion Vaporization. Heat of Fusion of Ice Lab.
Lab Quiz or Quiz as Exit Ticket Molar Heat of Solution Calculations. Heat of Solution Formation Lab. Given that 50 grams of ice is heated at -200 C to steam at 1350 C.
Show the graph of the changes from ice to steam ii. Calculate the energy needed to change the ice to steam Please use these values. Heat of fusion.
The calculation of the specific latent heat of fusion of ice is as follows. Heat lost by water is equal to the mass times the specific latent heat of fusion and the equation is VtIML M is mass of water in difference t stands for the time taken for heat the ice and L is the latent heat of fusion of ice. In this experiment you will try to measure the latent heat of fusion of ice LHice the energy needed per gram to melt ice.
The needed energy will come from a cup of warm water. The amount of water and its temperature will be measured before adding some ice and then again after the ice has been melted. This lab employs a double-wall calorimeter as shown in Figure 121 to measure the heat of fusion for ice.
The calorimeter consists of an aluminum container a reservoir a plastic lid and an insulator ring. The reservoir holds a maximum of 150 ml water. The clear plastic lid has 3 access holes.