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 equilibrium reaction has a very high K_c. The excess Fe^3+ prevents the formation of the neutral Fe(SCN)3. The reaction quotient Q is greater than K_c. The concentration of Fe(N0_3)_3 is much higher than the concentration of KSCN. Under the conditions given above, LeChaelier's principle dictates that the reaction shifts to the left.

Explanation / Answer

the equilibrium reaciton has a very high Kc value, meaning tha tproducts are strongly favoured

V = 9 ml of M = 0.2 Fe+3

V = 1 ml of M = 0.002 SCN-

the equilibrium concnetration must be approx that to the limiting reactant

i.e.

mol o Fe+3 = MV = 9*0.2= 0.18 mol of Fe+3

mol of SCN- = MV = 1*0.002 = 0.002 mol of SCN-

then SCN- is limiting

mol of FeCN+2 = 0.002

M = mol /L = 0.002/10 = 0.0002 M of FeSCN+2

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