Based on your description:
3) 55º-5º = 50º
5) (4.18J/g.ºC)(100.0g)(50º) = 20900 J
6) 20900J/75g = 278.7J/g
7) (278.7J/g)(18.0g/mol) = 5016 J/mole = 5.016 kJ/mol
8) %Error = (6.02-5.02)(100)/6.02 = 17%
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NOTE: Some of the heat lost by the warm water went into heating the melted ice from 0 deg C to 5.0 deg C. That was not taken into account in your procedure.
Hey,
for chemistry class we are given days in the lab to conduct an experiment, then answer a number of questions that correlate with that experiment and how we can make use of it. This week we looked at the Molar Fusion of Ice and there are some questions i don't quite understand.
The experiment went like this: water was poured into a beaker, heated (temperature and volume was taken), then cooled with ice cubes (temperature/volume taken again).
Here is my table of information:
volume of water after heated:100ml
temperature after heated:55ºC
temperature after cooled:.5ºC
Volume after cooled:175ml
Here are the questions:
1) Determine the volume of water in the ice-water mix that came from the melted ice.
2)Determine the mass of the water that came from the melted ice. Assume the density of water is 1.00g/ml
3)Determine the change in temperature of the warm water
4) Determine the mass of the warm water
5) Calculate the energy released by the warm water as it cooled through ΔT degrees (Hint: specific heat of water is 4.184J/gºC)
6) Calculate the energy released by the warm water for every gram of ice melted
7) Calculate the molar heat of fusion of ice (the kilojoules required to melt one mole of ice)
8) The accepted value for the molar heat of fusion of ice is 6.02. What is the percent error in the experimental value?
My Answers:
1 through 5 are mostly self-explanatory, the rest I'm pretty sure I'm doing them wrong
1) 75ml
2) 75g
3) -54.5ºC
4) 100g
5) q=CmΔT
q = 4.184(100)(-54.5)
q= -22802.8J
6) -22802.8/75=-304J
7) -22.8028kJ /18g=1.26
8) (1.26-6.02)/6.02*100=79%
umm.. yah.. can anyone help?
2 answers
Well I wrote the value .5 for the lowest temperatures but I think I will be able to use the equations you used anyway, thanks for the help!