Question

g Ions B and C react to form the complex BC. If 35.0 mL of 1.00 M B is combined with 35.0 mL of 1.00 M C, 0.00500 mol of BC is formed. Determine the equilibrium constant for this reaction.

Answer 1

Kf = 0.389.

Step-by-step explanation:

Hello there!

In this case, it turns out possible for us to solve this problem by firstly writing the equilibrium chemical equation and equilibrium expression for the formation of this complex:

`B+C\rightleftharpoons BC\\\\Kf=([BC])/([B][C])`

Thus, we firstly calculate the concentrations at equilibrium, knowing that the reaction extent in this case is 0.00500mol (same as the formed moles of BC):

`[B]=[C]=(0.0350L*1.00mol/L-0.00500mol)/(0.0700L) =0.429M`

`[BC]=(0.00500mol)/(0.0700L) =0.0714M`

And finally, the equilibrium constant:

`Kf=(0.0714)/([0.429][0.429])\\\\Kf=0.389`

Regards!