Answer:
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Explanation:
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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
- Write the given equation in ionic form
- Identify elements undergoing oxidation ( charge increase, O.N inc) and reduction (charge dec, O.N dec)
- Break the equation into two halfs
- 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)
N₂ → 2NO₃⁻
6H₂O + N₂ → 2NO₃⁻
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
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Moles Fe₂O₃ produced : 1.16 moles
<h3>Further explanation</h3>
Given
2.32 moles of iron
Required
moles of Fe2O3
Solution
The reaction coefficient in a chemical equation shows the mole ratio of the reacting compounds (reactants and products)
Reaction
4 Fe + 3 O₂ ⇒ 2 Fe₂O₃
From the equation, mol ratio Fe : mol Fe₂O₃ = 4 : 2, so mol Fe₂O₃ :
= 2/4 x mol Fe
= 2/4 x 2.32
= 1.16 moles