Question

In: Chemistry

Consider the following reaction: Fe3+(aq)+SCN−(aq)⇌FeSCN2+(aq) A solution is made containing an initial [Fe3+] of 1.1×10−3 M...

Consider the following reaction:
Fe3+(aq)+SCN−(aq)⇌FeSCN2+(aq)
A solution is made containing an initial [Fe3+] of 1.1×10−3 M and an initial [SCN−] of 8.2×10−4 M. At equilibrium, [FeSCN2+]= 1.8×10−4 M .

Part A

Calculate the value of the equilibrium constant (Kc).

Express your answer using two significant figures.

Kc=

Solutions

Expert Solution

                           Fe3+(aq)             +                SCN−(aq)⇌                          FeSCN2+(aq)

Initial                 1.1×10−3                                8.2×10−4                                                        0

Change             -1.8×10−4    -1.8×10−4    +1.8×10−4

At equilibrium    1.1×10−3 - 1.8×10−4                 8.2×10−4 - 1.8×10−4                   1.8×10−4   

Hence Kc = [FeSCN2+] / [Fe3+] [SCN−].

               =   [1.8×10−4] / [0.00092] [0.00064]

              Kc = 305.706


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