Problem: Using the standard reduction potentials, Pb 2+(aq) + 2e– => Pb(s), E° = –0.13 V Fe 2+(aq) + 2e– => Fe(s), E° = –0.44 V Zn 2+(aq) + 2e– => Zn(s), E° = –0.76 V which metal will reduce Mn 3+ to Mn 2+ (E° red = +1.51 V) but will not reduce Cr 3+ to Cr 2+ (E° red = -0.40 V)a. Pb onlyb. Fe onlyc. Zn onlyd. Fe and Zne. Fe and Pb

We're being asked to determine which metal/s are/is capable of reducing Mn³⁺ to Mn²⁺ but not Cr³⁺ to Cr²⁺ given their standard reduction potential

In this case, we have to get the resulting Ecell of each redox reaction pairing Mn³⁺/Mn²⁺ as well as Cr³⁺/Cr²⁺ to each oxidation of metal

Recall that the greater the E°_cell of a redox reaction, the more likely the reaction will occur (more spontaneous reaction)