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dsp73
3 years ago
7

What is the molar mass for N5O9

Chemistry
1 answer:
garik1379 [7]3 years ago
5 0

Answer:

The molar mass of N5O9

is 214.0245g/mol

Explanation:

To solve this problem, we need to know each number of mole of each element present in the compound

N has 5 moles

O has 9 moles

Then, we multiple each number of mole by its number of mass of each element present

N - 14.0067

O - 15.999

Multiplying by mole

N - 5 * 14.0067 = 70.0335

O - 9 * 15.999 = 143.991

Therefore,

Molar mass of N5O9 = 70.0335 + 143.991

= 214.0245g/mol

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The following steps are unbalanced half-reactions involved in the nitrogen cycle. Balance each half-reaction to show the number
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This is an oxidation reaction. The balanced equation is as follows:

      6H₂O  + N₂ → 2NO₃⁻+ 12H⁺  + 6e⁻

Rules to balance redox reaction in acidic medium

  1. Write the given equation in ionic form
  2. Identify elements undergoing oxidation ( charge increase, O.N inc) and reduction (charge dec, O.N dec)
  3. Break the equation into two halfs
  4. Balance the half equations

A. Balance all other atoms except Oxygen and hydrogen

B. Balance oxygen by adding H2O to the side deficient in oxygen

C. Balance hydrogen by adding H+ ions

D. Balance charge by adding electrons

5. Add the two half such that electrons gets cancelled

Oxidation number of N in N2 is 0 while in NO₃⁻, it is +5. Thus there is an increase in oxidation number, thus oxidation is taking place.

              N₂(g) → NO₃⁻(aq)

  • balance N.

           N₂ → 2NO₃⁻

  • balance O by adding H2O

          6H₂O  + N₂ → 2NO₃⁻

  • Now balance Hydrogen

            6H₂O  + N₂ → 2NO₃⁻+ 12H⁺

  • balance charge. 0 charge on left, -6 and + 12 on right. add 6e⁻ on right to balance.

             6H₂O  + N₂ → 2NO₃⁻+ 12H⁺  + 6e⁻

Thus we can conclude that since there is increase in oxidation number, oxidation is taking place.

learn more about balancing redox reactions at brainly.com/question/10203480

#SPJ4

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