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April 19, 2014

Homework Help: CHEMISTRY

Posted by Vanessa on Wednesday, April 21, 2010 at 4:55pm.

Hello, I am having trouble balancing this redox reaction WITHOUT using the half-reaction method. I believe this is because not all of the elements are in (aq).

BrO3-(aq) + N2H4(g) --> Br-(aq) + N2(g)

Br is reduced by a factor of 6.
N is oxidized by a factor of 2.

I will include these factors as coefficients and attempt to balance the hydrogen and oxygen.


2BrO3-(aq) + 6N2H4(g) --> 2Br-(aq) + 6N2(g)+ 6H2O(l)

It seems like I should be adding 12H+ to the products side to balance the hydrogen, but this doesn't work. I know the answer is:

2BrO3-(aq) + 3N2H4(g) --> 2Br-(aq) + 3N2(g)+ 6H2O(l)

But why are my stoichiometric factors incorrect for N2H4 and N2?

Thank you!

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