At a certain temperature K = 1.1 X 10^3 L/mol for the reaction given below. Calculate the concentrations of Fe3+, SCN?, and FeSCN2+ at equilibrium if 0.020 mol of Fe(NO3)3 is added to 1.0 L of 0.10 M KSCN. (Neglect any volume change.)Fe3+(aq) + SCN ?(aq) FeSCN2+(aq)Fe3+MSCN- MFeSCN2+ M

Explanation:

Fe⁺³ + SCN⁻ =  FeSCN²⁺

x           x                x

If x mole of Fe⁺³ reacted , unreacted Fe⁺³ = .02 - x

Remaining SCN⁻  unreacted = .1 - x

K_c =   [ FeSCN²⁺] / [Fe⁺³] [ SCN⁻]

1.1 x 10³ =  x  / ( .02 - x ) (.1 - x )

1100 = x / .002 - .12x ( neglecting x² )

x = .0165

Concentration of Fe⁺³ = .02 - x = .0035 M

Concentration of SCN⁻ = .1 - x = .0835 M

Concentration of FeSCN²⁺ = x = .0165M

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the positions which points up in upward carbon and down in downward carbon are axial

and vice versa holds true for equatorial positions

so the correct answer with labelled diagram will be