CHE 31 Lecture Notes - Chemical Equilibrium, Reversible Reaction, Partial Pressure
Document Summary
H2o (l) h2o(g) e r u s s e r p l a i t r a p c n o. The value of equilibrium constant for a reaction is constant at a particular temperature. There are two types of equilibrium reactions: homogeneous equilibrium. Here all reactants and products are in the same phase. Here all reactants and products are not in the same phase. 2 a (g) 2b(g) aa (g) + bb (g) cc (g) + dd (g) Write equilibrium constant expression (kp and kc) for the following reactions: n2(g) +3h2(g) Kp = kc (rt) n n = moles of gaseous products moles of gaseous reactants. T= temperature in kelvin aa (g) + bb (g) cc (g) + dd (g) n. 4 no(g) + 6 h2o(l) kc is 3. 5x105 at 400oc. If the equilibrium constant for the first reaction is k, write the equilibrium constant for the other two reactions.
