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A voltaic cell with Mn/Mn²⁺ and Cd/Cd²⁺ half-cells has the following initial concentrations: [Mn²⁺] = 0.090 M; [Cd²⁺] = 0.060 M(c) What is [Mn²⁺] when Ecell reaches 0.055 V?

Respuesta :

The concentration of manganese ion is 0.150 M

Using the Nernst equation, we can write as follows;

Ecell= E0 cell-0.0592/n logQ

logQ=Ecell- E0 cell/-0.0592V/n

log(Mn^+/Cd^2+)= 0.55V-0.7724V/-0.0592V/2

log(0.090+x/0.060-x)=24.2365

Taking logarithm both sides, we get

0.090+x/0.060-x=10^24.2365

x=0.06 M(on solving)

So the concentration of [Mn^2+] is 0.090+x=0.090+0.06=0.150 M

What is a voltaic cell?

  • A Voltaic Cell is a galvanic cell which is an electrochemical cell that uses spontaneous redox reactions to generate electricity. It consists of two separate half-cells.
  • A half-cell is composed of an electrode containing a strip of metal M within a solution containing M^n+ ions in which M is any arbitrary metal.

To learn more about voltaic cells visit:

https://brainly.com/question/1370699

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