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.
2007-03-05 11:58:29 · 4 answers · asked by Anonymous in Science & Mathematics ➔ Chemistry
25.11
2007-03-05 12:07:04 · answer #1 · answered by Anonymous · 0⤊ 0⤋
the guy above me has the properly desirable answer, besides the undeniable fact that the first man or woman to respond to that is faulty. First: The equation of Enthalpy of answer is H(sol)= - (lattice potential)+H(hydration) H=enthalpy So, change all of your numbers: H(sol)= - ( -715 ) + ( - 684) H(sol)=31 kJ/mol Then multiply this determination by technique of the variety of moles: 31 kJ/mol x a million.23 = 38.13 kJ/mol
2016-12-05 07:15:00 · answer #2 · answered by ? 4 · 0⤊ 0⤋
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2016-05-16 05:40:52 · answer #3 · answered by Anonymous · 0⤊ 0⤋
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.
2007-03-05 12:08:54 · answer #4 · answered by Anonymous · 1⤊ 0⤋