A standard solution of FeSCN^2+ is prepared by combining 6.00 mL of 0.00150 M Fe

Question

A standard solution of FeSCN^2+ is prepared by combining 6.00 mL of 0.00150 M Fe(NO_3)_3, 1.091 g KSCN, and deionized water in a 250 mL volumetric flask. The net ionic equation for the reaction is below. Fe^3+ + SCN^- Fe(SCN)^2+ What allows us to assume that the reaction goes essentially to completion? The concentration of KSCN is much higher than that of Fe(NO_3)_3. The equilibrium reaction has a very high K_c. the concentration of Fe(NO_3)_3 is much higher than the concentration of KSCN. The reaction quotient Q is greater than K_c. Under the conditions given above, LeChateller's Principle diciated that the reaction shifts to the left. Based on that assumption, what is the equilibrium constant of Fe(SCN)^2+? For clarification see the example calculation on page 7-5 your lab manual. Ince checked, the calculated molarity will be copied to the place for recording your work.

Explanation / Answer

Ans: The equilibrium has very high Kc.

If a reaction has high Kc i.e Kc >>>> 1 means the reaction is almost completed.

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