CHEMISTRY

Use the Nernst equation and data from Appendix D to calculate Ecell for each of the following cells.


Enter your answer with 3 significant digits.
Enter scientific notation as 1.23E4.



(a) Mn(s) | Mn2+(0.11) M || Cr3+(0.24 M), Cr2+(0.11 M) | Pt(s)

____________



(b) Mg(s) | Mg2+(0.070) M || [Al(OH)4]–(0.30 M), OH–(0.040 M) | Al(s)

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  1. a) Mn(s) | Mn2+(0.11) M || Cr3+(0.24 M), Cr2+(0.11 M) | Pt(s)

    1. Calculate4 the Mn^2+ + e ==> Mn couple.
    E = Eo - 0.0592/n)*log(red/(ox)
    E = Eo-(0.0592/n)*log[Mn(s)]/(Mn^2+)
    E = Eo = (0.0592/2)*log[(1)/(0.11)]
    You will need ot look up Eo for this REDUCTION, calculate E for the half cell, then change the sign since this is an oxidation.

    Do the same for the Cr^3+ + e ==> Cr^2+

    Then EMn as oxidation + ECr as redn = Ecell.

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