Question

Write the balanced equation for the nitrification reaction. Also write the half reactions used for the...

Write the balanced equation for the nitrification reaction. Also write the half reactions used for the final equation. Hint (Ox + ne^- + mH^+ ---> Red. + m/2 H20

Homework Answers

Answer #1

Nitrification is a process of nitrogen compound oxidation.

2 NH4+ + 3 O2 2 NO2 + 2 H2O + 4 H+

The oxidation states are mentioned below:

-3           0            +3              -2

2 NH4+ + 3 O2 2 NO2 + 2 H2O + 4 H+

Here the oxidation state of N increases from -3 to +3 so the oxidation half reaction is:

2 NH4+ 2 NO2

The oxidation state of O decreases from 0 to -2 so the reduction half reaction is:

3 O2 2 H2O

Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
For the reaction Si(s) + O2(g) --> SiO2(s): Write the balanced half cell redox reactions that...
For the reaction Si(s) + O2(g) --> SiO2(s): Write the balanced half cell redox reactions that could be used to measure the Ecell and Delta G. Label the oxidation and reduction half cell reactions
9) In the following equation, give balanced half reactions for each, the final combine reaction, and...
9) In the following equation, give balanced half reactions for each, the final combine reaction, and indicate the element that has been oxidized and the one that has been reduced. a. CO2 + NH2OH --> CO + N2 in basic solution. (show all work)
8. Use the following half-reactions to write a balanced full reaction for the reduction of iron...
8. Use the following half-reactions to write a balanced full reaction for the reduction of iron (II) by copper, and compute the standard electromotive force for this reaction (spectator ions are not required). Also calculate the Gibbs energy for this reaction! Cu+ + e − → Cu E◦ = +0.52 V (1) F e2+ + 2e − → F e E◦ = −0.44 V (2)
Write the balanced oxidation and reduction half reactions for reaction of Fe(II) with permanganate in acidic...
Write the balanced oxidation and reduction half reactions for reaction of Fe(II) with permanganate in acidic solution.
Depending upon the conditions, potassium permanganate may form Mn(s), Mn2+, or Mn3+. Write a balanced half-reaction...
Depending upon the conditions, potassium permanganate may form Mn(s), Mn2+, or Mn3+. Write a balanced half-reaction chemical equation for each reaction. Determine the number of electrons transferred and the equivalent mass of potassium permanganate for each condition. Also determine the molarity of a 0.200 M solution of KMnO4 assuming the final oxidation state of manganese if +2.
Nernst Equation Applied to Half-Reactions The Nernst equation can be applied to half-reactions. 1) Calculate the...
Nernst Equation Applied to Half-Reactions The Nernst equation can be applied to half-reactions. 1) Calculate the reduction potential (at 25°C) of the half-cell Cu/Cu2+ (1.5×10-2 M). (The half-reaction is Cu2+ + 2e- --> Cu.) 2) Calculate the reduction potential (at 25°C) of the half-cell MnO4- (1.80×10-1 M)/ Mn2+ (4.00×10-2 M) at pH = 6.00. (The half-reaction is MnO4- + 8H+ + 5e- --> Mn2+ + 4H2O.)
write out the two redox half-reactions (oxidation and reduction), and use half redox half-reactions to write...
write out the two redox half-reactions (oxidation and reduction), and use half redox half-reactions to write the balanced net ionic equation of Ag/Ag+ | | H+/H2 Cu/Cu2+ | | H+/H2 H2/H+ | | Zn2+/Zn Cu/Cu2+ | | Zn2+/Zn Ag/Ag+ | | Zn2+/Zn
A chemist designs a galvanic cell that uses these two half-reactions: half-reaction standard reduction potential Cl2(g)+2e−→...
A chemist designs a galvanic cell that uses these two half-reactions: half-reaction standard reduction potential Cl2(g)+2e−→ 2Cl−(aq)   E0red = +1.359V NO−3(aq)+4H+(aq)+3e−→ NO(g)+2H2O(l)   E0red = +0.96V Answer the following questions about this cell. Write a balanced equation for the half-reaction that happens at the cathode.   Write a balanced equation for the half-reaction that happens at the anode.   Write a balanced equation for the overall reaction that powers the cell. Be sure the reaction is spontaneous as written.   Do you have enough...
A chemist designs a galvanic cell that uses these two half-reactions: half-reaction standard reduction potential N2(g)+4H2O(l)+4e−→...
A chemist designs a galvanic cell that uses these two half-reactions: half-reaction standard reduction potential N2(g)+4H2O(l)+4e−→ N2H4(aq)+4OH−(aq) E0red = −1.16V Zn+2(aq)+2e−→ Zn(s) E0red = −0.763V Answer the following questions about this cell. Write a balanced equation for the half-reaction that happens at the cathode.   Write a balanced equation for the half-reaction that happens at the anode.   Write a balanced equation for the overall reaction that powers the cell. Be sure the reaction is spontaneous as written.   Do you have enough...
Write the balanced complete ionic equation for the reaction HI(aq)+CsOH(aq)→ Write the balanced net ionic equation...
Write the balanced complete ionic equation for the reaction HI(aq)+CsOH(aq)→ Write the balanced net ionic equation for the reaction HI(aq)+CsOH(aq)→ Write the balanced complete ionic equation for the reaction HCHO2(aq)+NaOH(aq)→ Write the balanced net ionic equation for the reaction HCHO2(aq)+NaOH(aq)→ Write the balanced complete ionic equation for the reaction HC2H3O2(aq)+LiOH(aq)→ Write the balanced net ionic equation for the reaction HC2H3O2(aq)+LiOH(aq)→ Express your answer as a chemical equation. Identify all of the phases in your answer.