The electrochemical reaction below at 25°C.
Ag⁺(0.275 M) + Fe²⁺(0.180 M) Fe³⁺(0.200 M) + Ag(s)

-Refer to Exhibit 17-3. What will be the concentration of Fe³⁺ when the reaction reaches equilibrium?

Question

The electrochemical reaction below at 25°C.
Ag⁺(0.275 M) + Fe²⁺(0.180 M)

The electrochemical reaction below at 25°C. Ag<sup>+</sup>(0.275 M) + Fe<sup>2+</sup>(0.180 M) Fe<sup>3+</sup>(0.200 M) + Ag(s) -Refer to Exhibit 17-3. What will be the concentration of Fe<sup>3+</sup> when the reaction reaches equilibrium? A) 0.183 M B) 0.217 M C) 0.112 M D) 0.290 M E) None of the above

Fe³⁺(0.200 M) + Ag(s)

-Refer to Exhibit 17-3. What will be the concentration of Fe³⁺ when the reaction reaches equilibrium?

Quizplus · Accepted Answer

The reaction is:Fe²⁺ + Ag⁺ → Fe³⁺ + AgThe equilibrium constant for this reaction is:K = [Fe³⁺][Ag]/[Fe²⁺][Ag⁺] = 1.56 x 10¹⁰At equilibrium, the concentrations of the reactants and products will be such that the value of K is equal to the equilibrium constant.Let x be the concentration of Fe³⁺ at equilibrium. Then, the concentration of Fe²⁺ will be 0.183 - x, the concentration of Ag⁺ will be 0.217 - x, and the concentration of Ag will be x.Substituting these values into the equilibrium constant expression, we get:1.56 x 10¹⁰ = x²/(0.183 - x)(0.217 - x)Solving for x, we get:x = 0.183 MTherefore, the concentration of Fe³⁺ at equilibrium will be 0.183 M.

The Electrochemical Reaction Below at 25°C