For the following process:
H2O(g) + Cl2O(g) à 2HOCl(g)
Ho(H2O(g))= 242KJ/mol Ho(Cl2O(g))=80KJ/mol Ho(HOCl(g))= -80KJ/mol
So(H2O(g))= 0.189 KJ/K So(Cl2O(g))=0.266 KJ/K So(HOCl(g))= 0.237
KJ/K
A) Calculate ΔHo, ΔSo and ΔGo
B)Calculate ΔG at 100K and P(H2O)=P(Cl2O)= P(HOCL)=10atm
(A)
ΔHorxn = 2 ΔHof(HOCl) - ΔHof (H2O) - ΔHo (Cl2O) = 2(-80) - (-242) - (80) = +2 kJ
ΔSorxn = 2 ΔSof(HOCl) - ΔSof (H2O) - ΔSo (Cl2O) = 2 (0.237) - 0.189 - 0.266 = + 0.019 kJ/K
ΔGo = ΔHorxn - TΔSorxn = + 2 - 298 (0.019) = - 3.662 kJ
(B)
ΔG = ΔGo + R T lnK
= ΔGo + R T lnPHOCl2/PH2O*PCl2O
ΔG = - 3.662 + (0.008314 * 373.15* ln(10)2/(10*10))
ΔG = - 3.662 kJ
For the following process: H2O(g) + Cl2O(g) à 2HOCl(g) Ho(H2O(g))= 242KJ/mol Ho(Cl2O(g))=80KJ/mol Ho(HOCl(g))= -80KJ/mol So(H2O(g))= 0.189...
At 25oc, Kc = 0.090 for the following reaction. H2O(g) + Cl2O(g) 2 HOCl(g) Calculate the equilibrium concentration of all species if the initial concentration of HOCl = 1.50 M. H2O(g) + Cl2O(g) 2 HOCl(g) Start Change Equil.
Consider the following reaction and the value of its equilibrium constant: H2O(g) + Cl2O(g) ⇌ 2HOCl(g) Keq = 0.090 If the equilibrium concentration of HOCl is measured at 0.15 M, what are the equilibrium concentrations of H2O and Cl2O, assuming that they are equal?
1. At 25oc, Kc = 0.090 for the following reaction. H2O(g) + Cl2O(g) 2 HOCl(g) Calculate the equilibrium concentration of all species if the initial concentration of HOCl = 1.50 M. H2O(g) + Cl2O(g) 2 HOCl(g) Start Change Equil.
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