Ask Question
3 June, 18:01

The following redox reaction is conducted with [Al3+] = 0.12 M and [Mn2+] = 1.5 M.

2 Al (s) + 3 Mn2 + (aq) → 2 Al3 + (aq) + 3 Mn (s) Eocell = 0.48 V Determine the moles of electrons transferred for the reaction as written (n), Q, and the cell potential (Ecell) at 298 K.

+3
Answers (1)
  1. 3 June, 19:02
    0
    0.47V

    Explanation:

    2 Al (s) + 3 Mn2 + (aq) → 2 Al3 + (aq) + 3 Mn (s)

    n = 6 (six moles of electrons were transferred)

    Q = [Red]/[Ox] but [Red] = 1.5M, [Ox] = 0.12 M

    Q = 1.5/0.12 = 12.5

    From Nernst equation:

    E = E°cell - 0.0592/n log Q

    E°cell = 0.48 V

    E = 0.48 - 0.0592/6 log (12.5)

    E = 0.47V
Know the Answer?
Not Sure About the Answer?
Get an answer to your question ✅ “The following redox reaction is conducted with [Al3+] = 0.12 M and [Mn2+] = 1.5 M. 2 Al (s) + 3 Mn2 + (aq) → 2 Al3 + (aq) + 3 Mn (s) Eocell ...” in 📙 Chemistry if there is no answer or all answers are wrong, use a search bar and try to find the answer among similar questions.
Search for Other Answers