Iron (III) ion and thiocyanate ion exists in equilibrium with iron thiocyanate ion. The reaction, as...

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Chemistry

Iron (III) ion and thiocyanate ion exists in equilibrium withiron thiocyanate ion. The reaction, as written, isexothermic. Given that theFeNCS²⁺
product is a deep red color and the reactants are nearly colorless,which of the following will cause the solution tobedarker in color at equilibrium?
Fe³⁺(aq) +NCS^â€“(aq) â†”FeNCS²⁺(aq)
Increasing the solution temperature
Adding FeNO₃
Removing Fe³⁺ ion by adding NaOH which reacts withFe³⁺ ion.
Removing NCS^â€“ ion by addingAgNO₃ with reactacts withNCS^â€“ ion.
None of these

Answer & Explanation Solved by verified expert

4.5 Ratings (675 Votes)

1 The reaction is exothermic in nature so on increasing the temperature the equilibrium will shift in reverse directionaccording to Le Chatliers principleIn exothermic reaction the reactants are higher in energy than the products so raising temperature See Answer

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		Increasing the solution temperature
		Adding FeNO₃
		Removing Fe³⁺ ion by adding NaOH which reacts withFe³⁺ ion.
		Removing NCS^â€“ ion by addingAgNO₃ with reactacts withNCS^â€“ ion.
		None of these