following data was collected after running a calorimetric experiment using three

Question

following data was collected after running a calorimetric experiment using three Table 1: AHsol Values of Salts Salt | Hsol (kJ/mol) LiI -63.60 -2.51 4.73 LiNO3 LiF The data collected for each experiment is as follows Experiment 1: 2.91 g of unknown salt added to 180, mL of water resulted in a value of-1.8°C. Experiment 2: 2.91 g of unknown salt added to 180. mL of water resulted in a value of-0.1°C. Experiment 3: 2.91 g of unknown salt added to 180. mL of water resulted in a T value of 0.7°C. Calculate the value of q for each of the experiments. (Assume that the heat capacity of water is 4.1801 J/g.°c.) Experiment 1 Experiment 2 4. Experiment 3 4 ent 2 9

Explanation / Answer

We know the formula Q = mCp Delta T

For experiment 1, Q = 2.91 x 4. 18 x -1.8 = -21.89J

For experiment 2, Q = 2.91 x 4. 18 x -0.1 = -1.22J

For experiment 3, Q = 2.91 x 4. 18 x 0.7 = 8.51J

so comparing the values and sign, Exeperiment 1 is LiI salt. Exeperiment 2 is LiNO3 salt. Exeperiment 3 is LiF salt .

the formula says DeltaH = delta q -delta (PV)

Since neither of the V or P is changing, deltaH = delta Q

So, Delta H sol = Q

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