A Standard solution of FeSCN^2+ is prepared by combining 9.0 mL of 0.20 M Fe(NO_

Question

A Standard solution of FeSCN^2+ is prepared by combining 9.0 mL of 0.20 M Fe(NO_3)_3 with 1.0 mL of 0.0020 M KSCN. The equation for the reaction is as follows. Fe(NO_3)_3 + KSCN FeSCN^2+ + KNO_3 + 2NO^-_3 What allows us to assume that the reaction goes essentially to completion? The reaction quotient Q is greater than K_c. 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 excess Fe^3+ prevents the formation of the neutral Fe(SCN)_3. Under the conditions given above, LeChatelier's principle dictates that the reaction shifts to the left. Based on that assumption, what is the equilibrium concentration of FeSCN^2+? M

Explanation / Answer

For the reaction: * reaction quotient Q is greater than Kc as equilibrium shifts to right *   the concentration of Fe(NO3)3 is much higher . * The excess Fe3+ prevents formation of neutral Fe(SCN)3. * reaction shifts to the Right .    * equilibrium Kc is very less.

equlibrium concentration of FeSCN is 0.0020 M as SCN comes from KSCN , concentration of KSCN is lowest in the reactant.

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