Question

The standard potential of electrode Cu⁺⁺(0.02 M) | Cu_(s) is 0.337 volt. Calculate its potential in volt.

Answer 1

For the half cell:

\[\ce{Cu^{2+} (0.02 M) + 2e- -> Cu_{(s)}}\]

Given:
Standard electrode potential, E° = 0.337 V

Concentration of Cu²⁺ = 0.02 M

Temperature = 298 K

Using the Nernst equation for the reduction reaction:

E = `E^circ - 0.0591/n log  1/([Cu^(2+)])`

= `0.337 - 0.0591/2 log  1/0.02`

= `0.337 - 0.0591/2 log(50)`

= `0.337 - 0.0591/2 xx 1.699`

= 0.337 − 0.02955 × 1.699

= 0.337 − 0.0502

= 0.287 V