In this question you will use your data from Table 8-2 provided below to determi

Question

In this question you will use your data from Table 8-2 provided below to determine DeltaHfusion for water for Part 1, Procedure 2 of the lab. Let's go through the calculations. Determine the absolute value of the heat "lost" by the water originally in the calorimeter in each trial. Please review your entries and make corrections where necessary. Part 5: Determine DeltaHfusion for water for each trial in units of kJ/mol. Determine the average value DeltaHfusion for water in units of kJ/mol. The acceptable value for DeltaHfusjon for water is 6.0 kJ/mol. Determine the percent error (absolute value) for your average value of DeltaHfusjon for water.

Explanation / Answer

#Trial 1

Mass of ice = 152.94-(29.58+99.58) = 23.78 g =1.32 moles

Moles of water = 29.58/18 = 1.64

Temp = 22 C

So, heat lost = (22-0)*29.58*4.2 J = 2733.192 J

Heat gained by ice = 2.733 kJ

Moles = 1.32

H fusion= 2.733/1.32 = 2.07 kJ/mol

#Trial 2

Mass of ice = 137.59-(29.58+99.58) = 8.43 g =0.468 moles

Moles of water = 29.58/18 = 1.64

Temp = 22.2 C

So, heat lost = (22.2-0)*29.58*4.2 J = 2758.04J

Heat gained by ice = 2.758 kJ

Moles = 0.468

H fusion=2.758/0.468 = 5.89 kJ/mol

Average value of H fusion = (5.89+2.07)/2 = 3.98 kJ/mol

%age error = (6-3.98)/6*100 = 33.667%

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