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

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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)

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Problem Details

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 only

b. Fe only

c. Zn only

d. Fe and Zn

e. Fe and Pb

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