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My 'third table data' has 3 values for gain/loss of heat in the water(J) calculated from Q=mc delta T- -843.17 (trial 1) -1098.65 (trial 2) -885.78...
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My "third table data" has 3 values for gain/loss of heat in the water(J) calculated from Q=mc delta T-

-843.17 (trial 1)

-1098.65 (trial 2)

-885.78 (trial 3)


trial 1: 4.221g (m), volume 106.32, initial temperature 48.23 degrees C, final temperature 0.43

trial 2: 5.397g (m), volume 108.97, initial temperature 49.22 degrees C, final temperature 0.52

trial 3: 4.353g (m), volume 107.43, initial temperature 49.07 degrees C, final temperature 0.47


I don't understand how to take these values and calculate the heat energy the melted the ice (which blocks me off from answering the other questions). Please help!


Use the equation, Qwater + Qf + Qmelted ice = zero & third table data to calculate the heat energy that melted the ice.


Use the equation, Qf = mLf and the data in your third table to calculate the heat of fusion of ice.


Report your experimentally-determined value of ΔH for the fusion of ice.


Was it necessary to include the Δ(PV) term in your calculations? Explain.


Use the Internet or a chemistry reference source, such as the CRC Handbook of Chemistry and Physics, to obtain the accepted value for the enthalpy of fusion of ice. If the given units are not J/g, perform a unit conversion to report the enthalpy of fusion in J/g.


Calculate the % error in your experimental enthalpy of fusion, compared with the accepted value.

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