Question

In a lab measuring electrochemical potential: - Would the measured potential of two electrodes of Cu/Cu^2+ (1M) and Cu/Cu^2+ (0.1M) be equal to, or different from, zero? Why? - Can the potentials that are measured in practice be considered standard potentials? Why? - What happens when we vary the concentration using the information given by the Nernst equation?

Name: in a lab measuring electrochemical potential would the measured potential of two electrodes of cucu2 1m and cucu2 1m be equal toor different from zero why can the potentials that are measure 96396
Uploaded: 2023-09-06T07:00:14-08:00
Duration: 1 min 51 s
Channel: Adi S
Description: in a lab measuring electrochemical potential would the measured potential of two electrodes of cucu2 1m and cucu2 1m be equal toor different from zero why can the potentials that are measure 96396

          In a lab measuring electrochemical potential:
- Would the measured potential of two electrodes of Cu/Cu^2+ (1M) and Cu/Cu^2+ (0.1M) be equal to, or different from, zero? Why?
- Can the potentials that are measured in practice be considered standard potentials? Why?
- What happens when we vary the concentration using the information given by the Nernst equation?

Added by Consuelo L.

Chemistry: Structure and Properties

Nivaldo Tro 2nd Edition

Instant Answer

Solved by Expert Adi S

09/06/2023

Step 1

The cell consists of two copper electrodes, each in a solution of Cu^2+ ions at different concentrations: one at 1M and the other at 0.1M. This setup forms a concentration cell. Show more…

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In a lab measuring electrochemical potential: - Would the measured potential of two electrodes of Cu/Cu^2+ (1M) and Cu/Cu^2+ (0.1M) be equal to, or different from, zero? Why? - Can the potentials that are measured in practice be considered standard potentials? Why? - What happens when we vary the concentration using the information given by the Nernst equation?