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April 18, 2014

April 18, 2014

Posted by **LaurenB** on Friday, December 2, 2011 at 4:02pm.

Species ΔfH (kJ/mol)

NaCl(aq)-407.3

NaCl(s) -411.2

- Thermochemistry -
**DrBob222**, Friday, December 2, 2011 at 9:27pmDH = delta H.

DHsoln = DHsolvation - DHlatticeenergy

DHsoln = -407.3 -(-411.2) = 3.9 kJ/mol

The + means it is an endothermic reaction and the water will become cooler; we are extracting heat from the water. How much? 3.9 kJ/mol x (1000 J/kJ) x 1.1 g NaCl x (1 mol NaCl/molar mass NaCl) = q and since we are extracting heat it is -q.

Then -q = mass H2O x specific heat H2O x (Tfinal-Tinitial) and solve for Tfinal.

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