In the reaction Fe 3 SCN Fe(NCS) 2 The initial concentration o...

Steps for calculating equilibrium constant are Write the e ....

In the reaction: Fe^3+ + SCN^âˆ’ â‡Œ [Fe(NCS)]2+ The initial concentration of Fe^3+ was 0.109 and the...

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Chemistry

In the reaction:
Fe^3+ + SCN^âˆ’ â‡Œ [Fe(NCS)]2+
The initial concentration of Fe^3+ was 0.109 and the initialconcentration of SCN^âˆ’ was 0.105. After equilibrium wasestablished, the concentration of the complex was 0.09. What is theequilibrium constant?

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3.6 Ratings (307 Votes)

Steps for calculating equilibrium constant are

Write the equilibrium expression for the reaction.
Determine the molar concentrations or partial pressures of each species involved.
Determine all equilibrium concentrations or partial pressures using an ICE chart.
Substitute into the equilibrium expression and solve for K

Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Fe ³⁺Â Â Â Â +Â Â Â Â SCN^âˆ’ â‡ŒÂ Â Â Â [Fe(NCS)]²⁺

Initial ConcentrationÂ Â Â Â Â Â Â Â Â Â Â Â 0.109Â Â Â Â Â Â Â 0.105Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â 0

Change in ConcentrationÂ Â Â Â Â -xÂ Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â - xÂ Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â =x

Equilibrium ConcentrationÂ Â Â Â 0.109- xÂ Â Â Â Â Â Â Â 0.105- xÂ Â Â Â Â Â Â Â Â 0.09

therefore x=0.09

Equilibrium ConcentrationsÂ Â Â 0.109-.09Â Â Â Â Â 0.105-0.09Â Â Â Â Â 0.09

Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â 0.019Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â 0.015Â Â Â Â Â Â Â Â Â Â 0.09

Hence, Equilibrium constant K_c = 0.09/0.019x0.015Â Â Â Â = 315 or 3.15 x 10²

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