chemistry

In a certain trial, the initial concentrations of Fe3+ and SCN- are both 1.00x10^-3 M and the initial concentration of FeSCN2+ is zero. Suppose that after the reation reaches equilibrium, the concentration of FeSCN2+ was found to be 1.19x10^-4 M. Use this information to calculate the value of Kc for the reaction, Fe3+ + SCN- <-> FeSCN2+. Show work.

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  1. Remember how to set up an ICE chart.
    .............Fe^3+ + SCN^- ==> FeSCN^2+
    initial.....0.001..0.001........0
    change........-x.....-x.........+x
    equil.....0.001-x...0.001-x...0.000119
    Therefore, x must be 0.000119
    Now you can calculate 0.001-x and plug into the Kc expression and solve for Kc.

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