Question

Can someone help me understand how to do a ICE table.

Use the ICE table to determine the equilibrium concentrations of the reactants and the equilibrium constant for this reaction.

Fe3+ +SCN- yields FeSCN2+

Fe3+ + SCN- yields FeSCN2+
Initial (M) 0.100 0.100 0
Change(M) -0.00361 -0.00361 +0.00361
Equilibrium(M) 0.09639 0.09639 0.00361

Kc=(FeSCN2+)/(Fe3+)(SCN-)
Kc=0.00361/(0.09639)(0.09639)
Kc=0.00361

This is what I have so far could someone please explain.