Consider the following half-reaction. 4H+(aq) + O2(g) + 4e- ? 2H2O(l) Eo = 1.23

Question

Consider the following half-reaction. 4H+(aq) + O2(g) + 4e- ? 2H2O(l) Eo = 1.23 V What is E, if the pressure of oxygen gas is 1.0 atmosphere and the pH is 7.68? USE 2 DECIMAL PLACES. (Hint, are solids and pure liquids included in Q? Using LeChatelier's principle is E going to be larger or smaller?)

Explanation / Answer

Nernst equation is apllied as follows: E = E° - RT/nF ln [M]/[M+] (for M+ --> M) where E = electrode potential under given concentration of M+ ions and temperature T E° = standard electrode potential R = gas constant = 8.314 J/K/mole T = temperature in kelvin F = 1 faraday = 96500 coulombs n = number of electrons involved in the electrode reaction pH = 7.68 -log [H+] = 7.68 log [H+] = -7.68 [H+] is calculated.

Related Questions

Navigate

• Browse (All)
• Browse C
• Subjects

---

---

Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.