Nernst Equation Applied to Half-Reactions

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SUMMARY

The Nernst equation is applicable to half-reactions, specifically for calculating reduction potentials. In the example provided, the reduction potential for the half-cell Cu/Cu2+ at a concentration of 1.9×10-4 M was calculated using the formula: E = E° - (RT/nF) * ln(Q). The correct calculation yields a reduction potential of 0.45 V, although the user initially received an incorrect result due to misinterpretation of the reaction quotient Q. The user later realized that the reaction quotient needed to be inverted for accurate results.

PREREQUISITES
  • Nernst Equation fundamentals
  • Understanding of half-reactions in electrochemistry
  • Basic logarithmic calculations
  • Knowledge of standard reduction potentials
NEXT STEPS
  • Study the derivation and applications of the Nernst Equation
  • Learn how to calculate reaction quotients for various half-reactions
  • Explore the impact of temperature on electrochemical reactions
  • Investigate common mistakes in electrochemical calculations
USEFUL FOR

Chemistry students, electrochemists, and anyone involved in calculating electrochemical potentials and understanding half-reactions.

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[SOLVED] Nernst Equation Applied to Half-Reactions

The Nernst equation can be applied to half-reactions.

Calculate the reduction potential (at 25°C) of the half-cell
Cu/Cu2+ (1.9×10-4 M).
(The half-reaction is Cu2+ + 2e- --> Cu. E° = 0.34 V)
0.34-[ (8.314)(298)/ (2)(96485)] * ln(1.9E-4)


This produces an answer of 0.45 V which I am confident is
the correct answer to this question but it says incorrect.
Am I approaching this question wrong, or doing the
calculations wrong?
 
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kadostan@hotmail.com

add me i did this one already but i need help on another, maybe u can help me, and if u need any maybe i have gotten!:S!
 
Last edited:
^^ sent you an email
 
nevermind...I got it. Forgot Q had to be flipped. Thanks though
 

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