Respuesta :
This is an incomplete question, here is a complete question.
An aqueous solution is made 1.000 M in AgNO₃ and 1.000 M in Fe(NO₃)₂ and allowed to come to equilibrium. What are the concentrations of the ions present when equilibrium is established.
[tex]Ag^+(aq)+Fe^{2+}(aq)\rightleftharpoons Ag(s)+Fe^{3+}(aq)[/tex]; K = 2.89
Answer : The concentration of [tex]Fe^{3+}[/tex], [tex]Fe^{2+}[/tex] and [tex]Ag^{+}[/tex] is, 0.565 M, 0.435 M and 0.435 M respectively.
Explanation :
The balanced chemical reaction is:
[tex]Ag^+(aq)+Fe^{2+}(aq)\rightleftharpoons Ag(s)+Fe^{3+}(aq)[/tex]
Initial: 1.000 1.000 0 0
At eqllm: (1.000-x) (1.000-x) x x
The equilibrium expression is:
[tex]K=\frac{[Fe^{3+}]}{[Ag^{+}][Fe^{2+}]}[/tex]
Now put all the given values in this expression, we get:
[tex]2.98=\frac{(x)}{(1.000-x)\times (1.000-x)}[/tex]
x = 0.565 M and x = 1.771 M
We are neglecting value of x = 1.771 because equilibrium concentration can not be more than initial concentration.
Thus, the value of x = 0.565 M
The concentration of [tex]Fe^{3+}[/tex] = x = 0.565 M
The concentration of [tex]Fe^{2+}[/tex] = (1.000-x) = (1.000-0.565) = 0.435 M
The concentration of [tex]Ag^{+}[/tex] = (1.000-x) = (1.000-0.565) = 0.435 M
The concentration of [tex]Fe^{3+},Fe^{2+} \text{ and } Ag^+[/tex] is 0.565 M, 0.435 M and 0.435 M respectively.
Balanced chemical reaction:
[tex]Ag^++Fe^{2+}---- > Ag+Fe^{3+}[/tex]
Initial: 1.000 1.000 0 0
At equilibrium: (1.000-x) (1.000-x) x x
The equilibrium expression is:
[tex]K=\frac{[Fe^{3+}]}{[Ag^+][Fe^{2+}]}}[/tex]
On substituting the values:
2.98 = (x) / (1.000-x) (1.000-x)
x = 0.565 M and x = 1.771 M
We are neglecting value of x = 1.771
Thus, the value of x = 0.565 M
The concentration of [tex]Fe^{3+}[/tex] = x = 0.565 M
The concentration of [tex]Fe^{2+}[/tex] = (1.000-x) = (1.000-0.565) = 0.435 M
The concentration of [tex]Ag^+[/tex]= (1.000-x) = (1.000-0.565) = 0.435 M
Find more information about Equilibrium constant here:
brainly.com/question/12858312
This is an incomplete question, here is a complete question.
An aqueous solution is made 1.000 M in AgNO₃ and 1.000 M in Fe(NO₃)₂ and allowed to come to equilibrium. What are the concentrations of the ions present when equilibrium is established.
[tex]Ag^++Fe^{2+}---- > Ag+Fe^{3+}[/tex]; K = 2.89
