The standard enthalpies of formation of ions in aqueous solutions are obtained by arbitrarily assigning a value of zero to H1 ions; that is, Hf[H1 (aq)] 5 0. (a) For the following reaction HCl(g) H2O H1(aq) 1 Cl2(aq) H 5 274.9 kJ/mol calculate DH8f for the Cl2 ions. (b) Given that DH8f for OH2 ions is 2229.6 kJ/mol, calculate the enthalpy of neutralization when 1 mole of a strong monoprotic acid (such as HCl) is titrated by 1 mole of a strong base (such as KOH) at 258C.
CHATER 11 ^IMF=^MP, ^BP, ^Viscosity, ^Surface Tension, vVP [S]Ion-D, H-Bond, D-D, Dis[W] vIMF=vMP, vBP, vViscosity, vSurface Tension, ^VP IMF, MM, Surface Tension= order of Prop. Ln(p2/p1)=(-DeltaH/R)(1/T2 – 1/T1) R=8.314 J/k.mol Q=n.DeltaH [no change in heat] Q=m.Cs.DeltaT T=C 1D=3.34e-30 C.m [S.D]S, L, G. [H-Bond]ration of 1 to 1 of lone pair and H, the more pairs the more higher/stronger. [G]Deposition[S]-DeltaH [S]Sublimation[G]+DeltaH [S]Melting[L]+DeltaH [L]Vaporization[G]+DeltaH [G]Condensation[L]-DeltaH [L]Freezing[S]-DeltaH DeltaH=KJ/mol DeltaHsub=DeltaHfus + DeltaHvap Equal VP= Evap and Conden even [Closed System] Normal Boiling Point= 1atm 1atm= 1/760torr (760torr) =760mmHg In(Pvap)=(-DeltaH/R)(1/T)+lnB Y=MX+B C+273.15K=K When given KJ use DeltaH to get mo
