CHEMISTRY

posted by .

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!

  • CHEMISTRY -

    The FIRST problem is that the loss of electrons for N2 is 4. N is +4 for the 2 N atoms and it goes to zero for the 2N atoms on the right. EACH N is -2 but you aren't dealing with EACH N. You are dealing with both on the left and both on the right.
    Second thing, not enough to start World War III over, but you should not say that Br changes by a factor of 6. It changes by 6 electrons, yes, and its a GAIN of 6e but not a FACTOR of 6.
    Br gains 6 electrons, both N change by 4 electrons. Multiply N by 6 and Br by 4 and see if things get easier.

Respond to this Question

First Name
School Subject
Your Answer

Similar Questions

  1. AP Chemistry

    i'm having trouble balancing the redox reaction for the iodine clock lab. The redox reaction inovlves a hydrogen sulfite ion and iodate ion in an acidified solution. i have the final balanced equation, 5 HSO3 + 2 IO3 ---> I2 + 5SO4 …
  2. CHEMISTRY

    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 …
  3. chemistry- redox

    Complete and balance the following equations using the method of half-reaction. both reactions happen in acidic solutions: a. Cu(s) + NO3-(aq)--> Cu2+(aq) + NO2(aq) b. Mn2+(aQ) + NaBiO3(s)--> Bi3+(aq) + MnO4-(aq) I'm having trouble …
  4. Chemistry

    1) Balance this redox reaction using the oxidation-number method. Zn + O2 + HCl ® ZnCl2 + H2O 2) Balance this redox reaction using the half-reaction method. (basic solution) Zn + MnO4- ® Zn(OH)2 + MnO2
  5. Chemistry

    I know nothing about chemistry, but am wondering if someone could help me with these. 1) Balance this redox reaction using the oxidation-number method. Zn + O2 + HCl ® ZnCl2 + H2O 2) Balance this redox reaction using the half-reaction …
  6. Chem

    How would one balance the following redox reaction using the half reaction method?
  7. Chemistry

    In a particular redox reaction, BrO– is oxidized to BrO3– and Cu2 is reduced to Cu . Complete and balance the equation for this reaction in acidic solution. Two half reactions: 1.) Cu^2+ --> Cu^+ 2.) BrO^- --> BrO3^- Balanced: …
  8. CHEMISTRY

    In half reaction method of the chemical equation balancing , how about those redox reactions that they don't contain any (H) and ( O ) atoms ?
  9. Chemistry

    Balance the redox reaction below using the half-reaction method. Bi3+(aq) + Co(s)Bi(s) + Co2+(aq)
  10. Chemistry

    Half reaction method of balancing redox reaction CHCl3 + MnO4- = Cl2 + CO2 + Mn+2

More Similar Questions