20) (17 points) Consider the following reaction: equation #2 MnCl5-2 (aq)  Mn+3 (aq) + 5 Cl-1 (aq)
(red) (yellow) (colorless)

a) At equilibrium, [ Mn+3 ] = 1.500 M, [ Cl-1 ] = 6.000 M, and [ MnCl5-2 ] = 2.750 M. Calculate the value of the equilibrium constant.

b) In another situation, [ Mn+3 ] = 5.000 M and [ MnCl5-2 ] = 2.000 M.
Calculate [ Cl-1 ].

Aqueous lead (II) ions react with aqueous chloride ions forming solid lead (II) chloride. The equation for this precipitation reaction is:

Pb+2 (aq) + 2 Cl-1 (aq)  PbCl2 (s)

Lead (II) ions are added to the solution that has equation #2.

c) Of the three chemicals in equation #2, which one of those chemicals will have its concentration directly affected by addition of lead (II) ions?

d) For that chemical in your answer to part ‘c’, is it a reactant or a product in equation #2?

e) For that chemical in your answer to part ‘c’, will its concentration increase or decrease with addition of lead (II) ions?

f) Based upon your answer from part ‘e’, which way will the equilibrium in equation #2 shift with addition of lead (II) ions?

g) Based upon your answer from part ‘f’, will the red color intensify and the yellow color fade, or will the red color fade and the yellow color intensify?

h) The solution that has equation #2 is placed in an ice water bath to lower the temperature of the equilibrium. One observes that the red color intensifies and the yellow color fades. Is this an exothermic reaction or an endothermic reaction?

Please answer c-h