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CH8_Page_08 - 3.32 8.34(a endothermically a positive...

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Unformatted text preview: 3.32 8.34 (a) endothermically: a positive enthalpy of solution means enthalpy is absorbed by the system during the dissolution process; (b) NH4N03(S] + heat 7—" NH“+ (aq) + NOE—[aqfi {(3) Given that nHL + AHMM = M of solution, the endothemue values of solution enthalpy result from systems with lattioe enthalpies greater than their enthalpies of hydration. Therefore, we expect that for Til-141N103 the lattice Cfllhflipy will be greater than the enthalpy of hydration. The molar enthalpies of solution are given in Table 8.6. Multiplying these numbers by the number of molm of solid dissolved will give the amount of heat released. The change in temperature will be given by dividing the heat: released by the speoifio heat capacity of the solution. (a) enthalpy ofsolution of K01 = +112 to atol—1 10.0 1; Kill _ 74.55 g-mol" KCl (4.1811K'lrg'1}(100.0 g} x (+172ooJ-mor') AT = = —5.52 K. or ~552°C {h} enthalpy of solution of ltngr2 = -185.6 kl whol—l MERE—x (—1ssaooJ-mor'} _ 134.13 glmol htthr2 [4.13 J -K'l -g'[){100.0 g) = +24.l K or +24.l ”C AT: (e) enthalpy of solution of END3 = +218 kJ -mo1" 10.0 g Knoj m _ (4.13 Lit-l -g"){l[li}.0 g) =—5.I53K.or 4.53%: x (+3300 .1 -rno1" J so" = (d) enthalpy of solution of NaOH = 44.5 kl . mot"I 1031} g NaCIH _ 4o.oo g -tuol_L NaOl-I (4.13 1-31" +g"}(it}0.fl g] = +2615 K or +26.6°C x {—44 500 J - mol'l) air = 234 ...
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