Can someone please show me how to do these calculations? The correct answers are
ID: 478640 • Letter: C
Question
Can someone please show me how to do these calculations? The correct answers are:
1) 22.6
2)4.87
3)2.0
Question Natalie Nimblefingers collected the following data in the enthalpy of fusion of ice experiment. 104.8 mL of water were initially at a temperature of 55.14 oC. After adding ice, the final temperature was 2.10 oC and the final volume Incorrect Grade 0.00 out of 174.9 mL. Calculate the heat required to melt the ice, q in kJ. Assume the density of water is 1.00 g/mL 2.00 Answer: 33.81 P Flag question Solving Equation (1) for qn gives q zCp abs(Tf TD ycp(Tf-273.15) where Cp 4.184 J/(gKl. Be sure to take the absolute value of the Temp difference. Note that z is the g of water initially and y is the g of ice melted where y (final g of water initial g of water) The correct number of significant figures is three The correct answer is: 22.6 Question 2 Elsa Iceheart calculated the heat (qp) required to melt 83.7 g of ice to be 22.61 kJ. Calculate the molar enthalpy of fusion of ice from this data in kJ/mol. Partially correct Grade 0.75 out of Answer: 4.66 1.00 P Flag questionExplanation / Answer
1. Heat required = q
Cp = 4.184 J/g.oC
final temperature of water = 2.10 oC
Initial temperature of ice = 0 oC
So,
q = 104.8 x 4.184 x (55.14 - 2.10) - (174.9 - 104.8) x 4.184 x 2.10/1000
= 23.876 kJ
2. Molar enthalpy of ice dHf
dHf = q/m
= 22610 x 18/83.7 x 1000
= 4.86 kJ/mol
3. percent error
Obtained dHf = 5.89 kJ/mol
% error = (5.89 - 4.86) x 100/5.89 = 17.50%