Select the single best answer. Consider the following half-reactions: MnO4 - (aq) + 8H + (aq) + 5e-→ Mn2 + (aq) + 4H2O (l) NO3 - (aq) + 4H + (aq) + 3e - → NO (g) + 2H2O (l) Will NO3 - oxidize Mn2 + to MnO4 - under standard-state conditions? NO3 - ions will oxidize Mn2 + to MnO4 - under standard state conditions. NO3 - ions will not oxidize Mn2 + to MnO4 - under standard state conditions.

Question

Aliyah

Chemistry

12 February, 04:12

Select the single best answer. Consider the following half-reactions: MnO4 - (aq) + 8H + (aq) + 5e-→ Mn2 + (aq) + 4H2O (l) NO3 - (aq) + 4H + (aq) + 3e - → NO (g) + 2H2O (l) Will NO3 - oxidize Mn2 + to MnO4 - under standard-state conditions? NO3 - ions will oxidize Mn2 + to MnO4 - under standard state conditions. NO3 - ions will not oxidize Mn2 + to MnO4 - under standard state conditions.

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Abraham Bishop · Answer 1

NO3 - ions will not oxidize Mn2 + to MnO4 - under standard state conditions.

Explanation:

The reduction potential of NO3^ - is + 0.96V while the reduction potential of MnO4^ - is + 1.51V. Hence looking at the reduction potential values stated above, NO3^ - will not oxidize Mn^2 + to MnO4^-.

The MnO4^ - having a greater reduction potential will be reduced to Mn^2 + while NO3^ - will be oxidized to NO.