Iron (III) ion and thiocyanate ion exists in equilibrium with iron thiocyanate i

Question

Iron (III) ion and thiocyanate ion exists in equilibrium with iron thiocyanate ion. The reaction, as written, is exothermic. Given that the FeNCS2+
product is a deep red color and the reactants are nearly colorless, which of the following will cause the solution to bedarker in color at equilibrium?
Fe3+(aq) + NCS–(aq) FeNCS2+(aq)

Increasing the solution temperature

Adding FeNO3

Removing Fe3+ ion by adding NaOH which reacts with Fe3+ ion.

Removing NCS– ion by adding AgNO3 with reactacts with NCS– ion.

None of these

Increasing the solution temperature

Adding FeNO3

Removing Fe3+ ion by adding NaOH which reacts with Fe3+ ion.

Removing NCS– ion by adding AgNO3 with reactacts with NCS– ion.

None of these

Explanation / Answer

Solution :-

Reaction is at equilibrium

So according to the Le Chateliers principle increasing temperature will shift the reaction to reactant side in exothermic reaction.

Increasing the concentration of the reactant shift the equilibrium to product side

Removing the product will shift the equilibrium to product side.

Therefore increasing the temperature of the solution will shift the equilibrium to the left side so the solution would not become darker.

Adding FeNO3 means it gives the Fe+ ion which is present at the product side therefore it will shift equilibrium to the reactant side so no darker color observed.

Removing Fe3+ by adding NaOH means the decrease in the reactant concentration therefore equilibrium will shift to the reactant side and no dark color observed.

Removing NCS- means decreasing the reactant concentration therefore it will shift the equilibrium to the reactant side so no dark color observed.

So the answer is none of these

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