The Average Keq Calculated: 129.7 M Using your average Keg value, please calcula

Question

The Average Keq Calculated: 129.7 M

Using your average Keg value, please calculated what the equilibrium concentrations of Fe3 (aq), SCN (a), and FeSCN2+ (ag) in a solution made by combining 10.00mL of 0.0020M Fe(NO3)s and 10.00mL of 0.0020M KSCN. Please show your calculations. [20 points) 7. ease show vour calculations Hint: Determine your initial concentrations, and then a formula for your equilibrium concentrations. Plug these into the Keq equation, rearrange, and solve for X using quadratic formula. Reject the root that yields a negative equilibrium concentration

Explanation / Answer

The reaction : Fe3+ + SCN- ---> FeSCN^2+

Keq = [FeSCN^2+]/[Fe3+][SCN-]

initial [Fe3+] in solution = 0.002 M x 10 ml/20 ml = 0.003 M

initial [SCN-] in solution = 0.002 M x 10 ml/20 ml = 0.003 M

let x be the change in concentration of substrate at equilibrium,

Keq = 129.7 = x/(0.003 - x)(0.003 - x)

129.7x^2 - 260.4x + 1.17 x 10^-3 = 0

x = 4.50 x 10^-6 M

Thus, equilibrium concentrations of,

[Fe3+] = 2.9955 x 10^-3 M

[SCN-] = 2.9955 x 10^-3 M

[FeSCN^2+] = 4.50 x 10^-6 M

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