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Problema 2

Problema 2. Ni +2 + Cl -  NiCl + log 10 K Cl = -0.43 Ni +2 + OH -  NiOH + log 10 K 1 = 4.1 Ni +2 + 2OH -  Ni(OH) 2 log 10 K 2 = 9.0 Ni +2 + 3OH-  Ni(OH) 3 - log 10 K 3 = 12.0 4Ni 2+ + 4OH -  Ni 4 (OH) 4 4+ log 10 K 44 = 28.3 muy peq. Balance de Ni

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Problema 2

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  1. Problema 2 Ni+2 + Cl- NiCl+ log10 KCl = -0.43 Ni+2 + OH- NiOH+ log10 K1 = 4.1 Ni+2 + 2OH-  Ni(OH)2log10 K2 = 9.0 Ni+2 + 3OH-  Ni(OH)3- log10 K3 = 12.0 4Ni2+ + 4OH-  Ni4(OH)44+ log10 K44 = 28.3 muy peq. Balance de Ni Balance de Cl Balance de OH Balance de H

  2. Adición de 10-3M NH4OH NiT = 10-3 M = [Ni2+]+[NiCl+]+[NiOH+]+[Ni(OH)2]+[Ni(OH)3-] = [Ni2+](1+KCl[Cl-]+K1[OH-]+K2[OH-]2+K3[OH-]3) ClT = 10-3 M = [Cl-]+ [NiCl+] = [Cl-](1+KCl[Ni2+]) OHT = 10-3+ 10-7 +  = [OH-]+[NiOH+]+2[Ni(OH)2]+3[Ni(OH)3-] = [OH-]+[Ni2+](1+K1[OH-]+2K2[OH-]2+3K3[OH-]3) HT = 10-7 +  = [H+] = Kw/[OH-] pH = 9.31, pero Ni(OH)2 precipitación a) Sin considerar la disociación o precipitación de níquel

  3. Adición de 10-3M NH4OH NiT = 10-3 M – (Ni)p = [Ni2+]+[NiCl+]+[NiOH+]+[Ni(OH)2]+[Ni(OH)3-] = [Ni2+](1+KCl[Cl-]+K1[OH-]+K2[OH-]2+K3[OH-]3) = Ksp/[OH-]2(1+KCl[Cl-]+K1[OH-]+K2[OH-]2+K3[OH-]3) ClT = 10-3 M = [Cl-]+ [NiCl+] = [Cl-](1+KCl[Ni2+]) OHT = 10-3+ 10-7 +  - 2(Ni)p= [OH-]+[NiOH+]+2[Ni(OH)2]+3[Ni(OH)3-] = [OH-]+[Ni2+](1+K1[OH-]+2K2[OH-]2+3K3[OH-]3) HT = 10-7 +  = [H+] = Kw/[OH-] pH =8.1, NiT = 5.06x10-4 a) Considerando la precipitación de níquel

  4. Considerando la disociación de amoniaco NH4+ NH3 + H+ NiT = 10-3 M = [Ni2+]+[NiCl+]+[NiOH+]+[Ni(OH)2]+[Ni(OH)3-]+[Ni(NH3)i] = [Ni2+](1+KCl[Cl-]+K1[OH-]+K2[OH-]2+K3[OH-]3+  Ki[NH3]i) ClT = 10-3 M = [Cl-]+ [NiCl+] = [Cl-](1+KCl[Ni2+]) OHT = 10-3+ 10-7 +  = [OH-]+[NiOH+]+2[Ni(OH)2]+3[Ni(OH)3-] = [OH-]+[Ni2+](1+K1[OH-]+2K2[OH-]2+3K3[OH-]3) HT = 10-7 +  +β= [H+] = Kw/[OH-] (NH4)T = 10-3 = [NH4+]+[NH3]+i [Ni(NH3)i] = [NH4+] + β β = Todo el amoniaco formado por disociación = NH3+ [Ni2+]i Ki[NH3]i pH  7.9

  5. Equilibrio y Cinética Equilibrio (fase y/o reacción) Hacia donde procede el sistema Cinética (intra- or interfase) Que tan rápido alcanza a llegar Fuerza motriz  lejanía de equilibrio Velocidad  Coeficientes de transporte o energía de activación

  6. Equilibrium Equilibrio predice: T Uniforme P Uniforme (sin barrera) Concentración Uniforme (misma fase) Potencial Químico Uniforme (multifase) Fuera de Equilibrio

  7. Difusión Provocada por Movimiento Browniano http://www.phy.ntnu.edu.tw/ntnujava/viewtopic.php?t=41

  8. Procesos Cinéticos y de Transporte • Intrafase Relativemente rápido si la energía de activación es baja Dependente del mezclado • Interfase Generalmente lento Dependente de las condiciones interfaciales Transporte de reactivos y productos a y desde el interfase ó superficie

  9. Esquema de reacción homogénea Esquema de reacción heterogénea

  10. Balances por componente – Reactor por lotes

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