What is really going on in solution is, of course, much more complex than this.

Question

What is really going on in solution is, of course, much more complex than this. reactions rarely go to completion. Instead, they tend to be reversible and go both forwards and backwards at the same time. To handle this sort of situation, we write equilibrium expressions, which involve product and reactant concentrations and allow us to product the actual concentrations of species in solution even with these backward reactions going on. For example, an interesting outcome of equilibrium is that disturbing an equilibrium by changing the concentration of a reactant or product has a predictable effect on the concentrations of everything else in solution. We saw this in lab when we studied the equilibrium between Fe^3+, SCN^-, and FeSCN^2+: The effect on the concentrations of these three species when various stresses are applied are as follows: indicate increases or decreases for each, comparing the final equilibrium

Explanation / Answer

Equilibrium constant Keq = Concentration of products at equilibrium / Concentration of reactants at equilibrium

1) N2O4 (g) <----------> 2 NO2 (g)

Keq = [NO2]2 / [N2O4]

2) Sn(s) + 2NaOH (aq) <------------> Na2SnO2 (aq) + H2(g)

Total ionic equation : Sn(s) + 2Na+ (aq) + 2OH- (aq) <------------> 2Na+ (aq) + SnO22-(aq) + H2(g)

Net ionic equation: Sn(s) + 2OH- (aq) <------------>  SnO22-(aq) + H2(g)

Solids cannot be considered while calculating Keq .

   Keq = [ SnO22-] [H2]/ [OH-]2

  

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