Yes, you have set up the ICE table correctly for the given reaction. The initial concentrations of Fe^3+ and SCN^- are both 1.0M, and the concentration of Fe(SCN)^2+ at equilibrium is 5.7e-5M.
In the ICE table, you correctly assign the initial concentrations of Fe^3+, SCN^-, and Fe(SCN)^2+ under the columns I (Initial), C (Change), and E (Equilibrium). Since the stoichiometry of the reaction is 1:1:1, the change in concentration for Fe(SCN)^2+ is equal to the equilibrium concentration. Therefore, you correctly put 0 under the Change column for Fe(SCN)^2+.
For the concentrations of reactants at equilibrium, you correctly calculate that Fe^3+ is 0.99M and SCN^- is 0.99M by subtracting the equilibrium concentration of Fe(SCN)^2+ from the initial concentration of Fe^3+ and SCN^-.
However, when calculating the concentration of Fe^3+ at equilibrium, your calculation of 1.0 - 5.7e-5 gives you the value of 0.999943, not 0.99. This appears to be a calculator error or a typographical error in your submission. The correct calculation should yield 0.99.
Lastly, when calculating Kc, you correctly write the expression Fe(SCN) / [Fe][SCN] and substitute the given values to obtain Kc = 5.7e-5M / (0.99M)(0.99M) = 5.8e-5. So, overall, you have set up and solved the problem correctly.
Please double-check your calculations for the concentrations of reactants at equilibrium to ensure the correct values are used in further calculations.