Calculate the enthalpy of solution (KJ) of 0.810 moles of KCl.?
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The lattice energy of KCl(s) is −715 KJ/mol, and the enthalpy of hydration is −684 KJ/mol. Calculate the enthalpy of solution (KJ) of 0.810 moles of KCl.
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Answer:
It's -684 - (-715) = +31kJ/mol (so it's endothermic, NOT exothermic) So it's .81 * 31 = 25.11 kJ Huh? It's positive? That's because it's driven by entropy...the change in Gibbs free energy in negative because delta S is positive. If you don't know what Gibbs Free Energy is don't worry aboutit, you'll learn about that soon.
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