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Oxidation Number Method

Which one is ...

Question

Which one is balanced net ionic equations for the following reactions in acidic solution:
$H N O_{2} (a q) \to N O_{3}^{-} + N O (g)$

A

3 H N O_{2} (a q) \to N O_{3}^{-} (a q) + 2 N O (g) + H_{2} O + H^{+} (a q)

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B

4 H N O_{2} (a q) \to 3 N O_{3}^{-} + 2 N O (g) + H_{2} O + H^{+} + e^{-}

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C

3 H N O_{2} (a q) \to N O_{3}^{-} + 2 N O (g) + H_{2} O + H^{+} + e^{-}

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D

4 H N O_{2} (a q) \to N O_{3}^{-} + 2 N O (g) + H_{2} O + H^{+} + e^{-}

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Solution

The correct option is A $3 H N O_{2} (a q) \to N O_{3}^{-} (a q) + 2 N O (g) + H_{2} O + H^{+} (a q)$
Steps for Balancing redox reactions:

Identify the oxidation and reduction half .

Find the oxidising and reducing agent.

Find the n-factor of oxidising and reducing agent.

Balance atom undergoing oxidation and reduction.

Cross multiply the oxidising or reducing agent with n-factor.

Balance atoms other than oxygen and hydrogen.

Balancing oxygen atoms

Balancing hydrogen atoms

Balance charge

For acidic medium:
As soon as we add x $H_{2} O$ units, we add 2x $H^{+}$ ions on the opposite side.

$n_{f} = (| O . S ._{P r o d u c t} - O . S ._{R e a c t a n t} | \times number of atom$
$+ 3 H N O_{2} (a q) \to + 5 N O_{3}^{-} + + 2 N O (g)$
$+ 3 H N O_{2} (a q) \to + 5 N O_{3}^{-}$ oxidation
$n_{f} = (| 5 - 3 | \times 1 = 2$
$+ 3 H N O_{2} (a q) \to + 2 N O (g)$ reduction
$n_{f} = (| 2 - 3 | \times 1 = 1$

Balance atom undergoing oxidation and reduction.
$3 H N O_{2} (a q) \to N O_{3}^{-} + 2 N O (g)$

Balance oxygen atom.
$3 H N O_{2} (a q) \to N O_{3}^{-} (a q) + 2 N O (g) + H_{2} O$

Balance hydrogen.
$3 H N O_{2} (a q) \to N O_{3}^{-} (a q) + 2 N O (g) + H_{2} O + H^{+} (a q)$

balance charge
charge in reactant side = 0
charge in product side = 0
so the balanced equation is $3 H N O_{2} (a q) \to N O_{3}^{-} (a q) + 2 N O (g) + H_{2} O + H^{+} (a q)$

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Similar questions

Q. The number of redox reactions from the following equations are:
a.

H_{2} S + {F e}^{3 +} ⟶ {F e}^{2 +} + S ↓ + H^{\oplus}

I^{⊖} + I O_{3}^{⊖} + H^{\oplus} ⟶ I_{2} + H_{2} O

B i (s) + N O_{3}^{⊖} + H^{\oplus} ⟶ N O_{2} + {B i}^{3 +} + H_{2} O

I^{⊖} + O_{2} (g) + H_{2} O ⟶ I_{2} + ⊖ O H

C u (s) + {A u}^{\oplus} ⟶ A u (s) + {C u}^{2 +}

Q. The balanced equation for the reaction

N O_{3}^{-} + F e^{2 +} + H^{+} \to N O + F e^{3 +} + H_{2} O

Q. Balance the following equations by ion electron method.
a.

{C r}_{2} O_{7}^{2 -} + C_{2} H_{4} O + H^{\oplus} ⟶ 2 {C r}^{3 +} + C_{2} H_{4} O_{2} + H_{2} O

{C u}_{2} O + H^{\oplus} + N O_{3}^{⊖} ⟶ {C u}^{2 +} + N O + H_{2} O

Q. Balance the following equations by oxidation number method.

{C r_{2} O_{7}}^{2 -} + H N O_{2} + H^{+} \to C r^{3 +} + {N O_{3}}^{-} + H_{2} O

Q. Balance the following equation by ion electron method-

C u_{2} O + H^{+} + N O_{3}^{-} \to C u^{2 +} + N O + H_{2} O

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