Chemical Forums
Chemistry Forums for Students => High School Chemistry Forum => Topic started by: theguy on February 20, 2012, 12:28:19 PM
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I'm having trouble balancing a redox equation.
Specifically the half reaction method.
The equation is NH3 + NO2- :rarrow: N2 + H2O
No matter how many times I attempt this, I can never seem to get a reasonable answer.
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If there is no negative charge between products, you won't be able to balance this equation.
Are you sure it is not NH4NO2 decomposition?
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Okay, I misread the equation. There is no negative charge. It was just a stray mark on my paper. Nonetheless, I've worked it without the negative and still can't get an answer that makes sense.
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Not every reaction can be balanced. What you wrote is one of these cases without an answer. Compare http://www.chembuddy.com/?left=balancing-stoichiometry&right=balancing-failure
As I suggested earlier, most likely it should be NH4NO2, not NH3NO2.
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Not every reaction can be balanced. What you wrote is one of these cases without an answer. Compare http://www.chembuddy.com/?left=balancing-stoichiometry&right=balancing-failure
As I suggested earlier, most likely it should be NH4NO2, not NH3NO2.
The reactants aren't supposed to be combined. It's NH3 + NO2.
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Ok
check these two balanced half reactions for the reaction given by you
2NH3---> N2 + 6e- + 6H+
8H+ + 6e- + 2NO2- --------.> N2 + 4H2O
FINAL EQUATIONS IS
2NH3+ 2H+ + 2NO2- ---> 2N2 + 4H2O
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No
FINAL EQUATIONS IS
NH3 + H+ + NO2- ---> N2 + 4 H2O
But above it was written there was no negative Charge on NO2
So the reduction would be
2 NO2 + 8 H+ + 8 e- => N2 + 4 H2O
8 NH3 => 4 N2 + 24 e- + 24 H+
6 NO2 + 24 H+ + 24 e- => 3 N2 + 12 H2O
Final would be:
8 NH3 + 6 NO2 => 7 N2 + 12 H2O
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No
FINAL EQUATIONS IS
NH3 + H+ + NO2- ---> N2 + 4 H2O
But above it was written there was no negative Charge on NO2
So the reduction would be
2 NO2 + 8 H+ + 8 e- => N2 + 4 H2O
8 NH3 => 4 N2 + 24 e- + 24 H+
6 NO2 + 24 H+ + 24 e- => 3 N2 + 12 H2O
Final would be:
8 NH3 + 6 NO2 => 7 N2 + 12 H2O
I balanced this equation -
NH3 + NO2- ----> N2 + H2O
in this equation NO2 has -ve charge
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In the third post it was written:
Okay, I misread the equation. There is no negative charge. It was just a stray mark on my paper
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8 NH3 + 6 NO2 => 7 N2 + 12 H2O
Apparently I did something wrong before, as this is the correct answer.
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I'm not sure if I'm right, but I got
8NH3 + 14NO2 + 32H+ -> 11N2 + 28H2O
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I'm not sure if I'm right, but I got
8NH3 + 14NO2 + 32H+ -> 11N2 + 28H2O
Charges are unbalances