Balance the following redox equation which occurs in acidic solution. N2H4(g) + BrO3–(aq) → Br–(aq) + N2(g)

Question

Balance the following redox equation which occurs in acidic solution. N2H4(g) +  BrO3–(aq) →  Br–(aq) +  N2(g)

BlackTom AI · Accepted Answer

Oxidation states: N in N2H4 is -2 (each H is +1 so two N sum to -4 → -2 each) and Br in BrO3– is +5. N is oxidized (-2 → 0) and Br is reduced (+5 → -1). In acidic solution use H2O and H+ and balance electrons with half-reactions.

1) Relevant concepts
- Assign oxidation numbers to identify oxidation and reduction.
- Balance atoms (other than O and H), then O by H2O, H by H+, and charge by electrons.
- Multiply half-reactions to equalize electrons and combine.

2) Half-reactions and stepwise balancing
Oxidation (hydrazine → N2):
N2H4 → N2
Balance H by adding 4 H+ on right: N2H4 → N2 + 4 H+
Balance charge by adding electrons: left charge 0, right charge +4 so add 4 e– to right:
N2H4 → N2 + 4 H+ + 4 e–

Reduction (bromate → bromide):
BrO3– → Br–
Balance O by adding 3 H2O on right: BrO3– → Br– + 3 H2O
Balance H by adding 6 H+ on left: BrO3– + 6 H+ → Br– + 3 H2O
Balance charge by adding electrons: left charge (-1 +6 = +5), right -1, so add 6 e– to left:
BrO3– + 6 H+ + 6 e– → Br– + 3 H2O

3) Equalize electrons (LCM of 4 and 6 is 12)
Multiply oxidation half by 3:
3 N2H4 → 3 N2 + 12 H+ + 12 e–
Multiply reduction half by 2:
2 BrO3– + 12 H+ + 12 e– → 2 Br– + 6 H2O

4) Add and cancel (electrons and 12 H+ cancel)
3 N2H4 + 2 BrO3– → 3 N2 + 2 Br– + 6 H2O

5) Why this is correct
Check atoms and charge: N: 3·2 = 6 on both sides; H: 3·4 = 12 = 6·2; O: 2·3 = 6 = 6·1; Br: 2 each side. Charge: left 2(–1) = –2; right 2(–1) = –2. Fully balanced in acidic solution.

6) Why other choices are incorrect (brief)
- a) Wrong coefficients and places for H+ and H2O; atoms/charge not balanced.
- c) Adds 12 H+ on left but gives only 3 H2O on right — H and O do not balance.
- d) Incorrect stoichiometric factors; N and H counts don’t match.

Conclusion: The balanced equation is 3N2H4(g) + 2BrO3–(aq) → 2Br–(aq) + 3N2(g) + 6H2O(l), which matches answer b.

Balance the following redox equation which occurs in acidic solution. N2H4(g) + BrO3–(aq) → Br–(aq) + N2(g)Single choice

Similar Questions

Given the following redox reaction, write out the half-reaction that occurs at the anode and the cathode. Ni2+ (aq) + Mg (s) → Ni (s) + Mg2+(aq)

Balance the following redox reaction if it occurs in acidic solution. What are the coefficients in front of H2C2O4 and H2O in the balanced reaction? MnO4⁻(aq) + H2C2O4(aq) → Mn2+(aq) + CO2(g)

What element is being reduced in the following redox reaction? MnO4⁻(aq) + H2C2O4(aq) → Mn2+(aq) + CO2(g)

Indicate whether the following reactions are oxidation reactions, reduction reactions or neither. 1: 2: 3:

Under acidic conditions the bromate ion (BrO3–) is reduced to the bromide ion. The balanced half-equation for this process is:

Iodide ion reacts with manganese(IV) oxide according to: MnO2(s) + 2 I– (aq) + 4 H+(aq) → I2(aq) + Mn2+(aq) + 2 H2O(l) Which statement correctly describes this reaction?

The only redox reaction among the following is:

More Practical Tools for Students Powered by AI Study Helper

Homework AI Solver

Stylized AI Paper Writer

Plagiarism Checker Assistant

Citation AI Academic Writing Tool

In-Class Translation Assistant

AI Note Generator

AI Quiz Answers

Past Exam Questions from University Test Bank

Smart Practice Assistant

Adaptive Practice

Making Your Study Simpler