The formation of the iron(III) thiocyanate complex ion is an exothermic equilibrium system. For each change to the system, indicate how the concentration of each species in the chemical equation will change to reestablish equilibrium. An up arrow indicates an increase in concentration, a down arrow indicates a decrease in concentration, and leaving it blank means there is no change in the concentration.

Since the formation of Fe(SCN)²⁺ is an exothermic reaction (delta H is negative); an increase in temperature will favor the backward reaction and more reactants will be produced. When the temperature is however reduced, the forward reaction will be favored and more products will be produced.

When the concentration of the reactants increases, the forward reaction is favored and hence more Fe(SCN)²⁺ is produced. However, when the concentration of Fe(SCN)²⁺ decreases, the backward reaction is favored and more reactants are produced.

pstnonsonjoku pstnonsonjoku · Answer 2 · 2021-11-16T19:06:42+01:00

The conditions of the reaction determines the relative concentration of species in the system.

When a constraint is imposed on a reaction system in equilibrium, the equilibrium position will shift so as to annul the constraint. When the concentration of Fe^3+ is increased, concentration of SCN^- decreases while the concentration of FeSCN^2+ increases.

When the concentration of FeSCN^2+ decreases, the concentration of Fe^3+ and SCN^- decreases as well. Since the reaction is exothermic, increasing the temperature will lead to a decrease in the concentration of FeSCN^2+ and increase in the concentration of Fe^3+ and SCN^- .

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