Consider the following reaction: Fe3+( a q )+SCN( a q )FeSCN2+( a q ) A solution

Question

Consider the following reaction:
Fe3+(aq)+SCN(aq)FeSCN2+(aq)
A solution is made containing an initial [Fe3+] of 1.0×103 M and an initial [SCN] of 8.1×104 M . At equilibrium, [FeSCN2+]= 1.8×104 M .

Part A

Calculate the value of the equilibrium constant (Kc).

Consider the following reaction:
Fe3+(aq)+SCN(aq)FeSCN2+(aq)
A solution is made containing an initial [Fe3+] of 1.0×103 M and an initial [SCN] of 8.1×104 M . At equilibrium, [FeSCN2+]= 1.8×104 M .

Part A

Calculate the value of the equilibrium constant (Kc).

Explanation / Answer

                             Fe3+                    SCN-                       Fe(SCN)2+

Initial                  0.001                     0.0008                           0

equilibrium         0.001-X                  0.0008-X                          X

given X = 0.00018 , hence [Fe3+] = 0.001-0.00018 = 0.00082 , [SCN-]= 0.00062

K = [Fe(SCN)2+] /[Fe3+] [SCN-]

   = (0.00018 /0.00082 x 0.00062) = 354

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