   Chapter 13, Problem 76AE

Chapter
Section
Textbook Problem

# At a certain temperature, K = 9.1 × 10-4 for the reaction FeSCN 2 + ( a q ) ⇌ Fe 3 + ( a q ) + SCN − ( a q ) Calculate the concentrations of Fe3+, SCN-, and FeSCN2+ in a solution that is initially 2.0 M FeSCN2+.

Interpretation Introduction

Interpretation: The equilibrium constant and initial concentration of reactant for a given reaction is given. The value of concentration of all species is to be calculated.

Concept introduction: The state when the reactants involved in a chemical reaction and the products formed in the reaction exist in concentrations having no further tendency to change is known as an equilibrium state of the reaction.

For a reaction,

jA+kBlC+mD

The equilibrium constant is given by,

K=[C]l[D]m[A]j[B]k

To determine: The equilibrium concentration of [Fe3+] , [SCN] and [FeSCN2+] for the given reaction.

Explanation

Explanation

Given

The equilibrium constant is 9.1×104 .

The initial concentration of reactant is 2.0M .

The given reaction is,

FeSCN2+(aq)Fe3+(aq)+SCN(aq)

The initial concentration of product Fe3+ and SCN is zero.

It is assumed that the change in concentration of FeSCN2+ is x .

Make the ICE table for the given reaction.

FeSCN2+(aq)Fe3+(aq)SCN(aq)Initial(M):2.000Change(M):xxxEquilibrium(M):2.0xxx

At equilibrium, the equilibrium constant is expressed by the formula,

K=ConcentrationofproductsConcentrationofreactants

Where,

• K is the equilibrium constant.

The equilibrium constant for the given reaction is,

K=[Fe3+][SCN][FeSCN2+]

Substitute the value of K and equilibrium concentration values in the above expression

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