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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(b) What is Ecell when [Cd²⁺] reaches 0.050 M?

Respuesta :

The value of Ecell is 0.7724V

The reaction is Mn(s)+Cd^2+(aq)⇒Mn^2+(aq)+Cd(s)

Q=[Mn^2+]/[Cd^2+]=0.090/0.050=1.8

Using the Nernst equation, we can write as follows;

Ecell= E0 cell-0.0592/n logQ

Substituting the values, we get

Ecell=0.78-0.0592/2 log(1.8)

Ecell=0.7724 V

So the Ecell is 0.7724V

  • A Voltaic Cell is defined as a galvanic cell also called 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:

brainly.com/question/1370699

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