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Posted by on Thursday, April 22, 2010 at 5:07pm.

Hello, I am trying to balance this redox reaction WITHOUT using the half-reaction method. Here is the unbalanced equation:

MnO4 -(aq) + Zn(s)--> Mn 2+(aq) + Zn 2+(aq)

It looks as if both elements are being oxidized. The answer is supposed to be:

2MnO4 -(aq) + 16H +(aq) + 5Zn(s) --> 2Mn 2+(aq) + 8H2O(l) + 5Zn 2+(aq)

Thank you!

  • CHEMISTRY - , Thursday, April 22, 2010 at 5:12pm

    Mn goes from +7 on the left to +2 on the right so it is gaining 5e which is reduction. Zn is zero on the left and +2 on the right which is a loss of 2e which is oxidation. I helped you do one yesterday. I assume the corrections I made made it much easier to balance. Let me know if this one gives you any problems.

  • CHEMISTRY - , Thursday, April 22, 2010 at 6:18pm

    thank you so much! no, I've been doing many questions on half cells and cell potential and I mindlessly forgot to assign oxidation numbers, just going by the sign of the element as you would with half cell questions. you're awesome help! thanks!

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