HW 7-8: Question 5

[Shaniya Kerns 4D]

Can someone help me balance the reaction.
Identify the oxidizing and reducing agents in the skeletal (unbalanced) reaction. Then, balance the reaction, including the phase (solid, liquid, etc.) of each species. The reaction takes place in basic aqueous solution.
N2H4(g) + ClO3^-(aq) → NO(g) + Cl^- (aq)

balanced equation:
80H- + N2H4 + CIO3^- → 2NO + 3Н2O + CI- + 6OH

[April_Tello_2H]

Always remember that no matter what in acidic conditions you can add H+ and H20 to your equation to help you balance it out, but then you would have to equal it to the other side when writing the final redox reaction. After wards you will change to acidic by canceling your H+ with the OH-.

80H- + N2H4 + CIO3^- → 2NO + 3Н2O + CI- + 6OH

In this case you can start of with ClO3^- -> Cl^-, the charges are equal but you have 3 oxygen on the left side so you can add 3H2O to the right side to even out your oxygen. You can then add 6H+ to your left side so then equal the hydrogen amount, but then by doing this you have a positive 5 charge on the right and a negative 1 charge on the left, in this case you add your electron to the left side making it 6e- and now the charges are equal, this is the cathode, then do a similar process to the anode.

[Charlotte Norris 2K]

The balanced equation is: 3N2H4(g)+4ClO−3(aq) --> 6NO(g)+6H2O(l)+4Cl−(aq)