You visited us 1 times! Enjoying our articles? Unlock Full Access!

Redox Reactions and Couple

Which of the ...

Question

Which of the following represents the oxidation half-reaction for the unbalanced redox equation?
$C u + H N O_{3} \to C u (N O_{3})_{2} + N O_{2}$

C u^{2 +} + 2 e^{-} \to C u

No worries! We‘ve got your back. Try BYJU‘S free classes today!

C u \to C u^{2 +} + 2 e^{-}

Right on! Give the BNAT exam to get a 100% scholarship for BYJUS courses

N O_{3}^{-} \to N O_{2} + 1 e^{-}

No worries! We‘ve got your back. Try BYJU‘S free classes today!

2 H^{+} + N O_{2}^{-} + 1 e^{-} \to N O_{2} + H_{2} O

No worries! We‘ve got your back. Try BYJU‘S free classes today!

Open in App

Solution

The correct option is B $C u \to C u^{2 +} + 2 e^{-}$
$C u + H N O_{3} ⟶ C u (N O_{3})_{2} + N O_{2}$
As Oxidation of $C u$ is taking place in the reaction.
Thus the oxidation half-cell reaction will be $C u ⟶ C u^{+ 2} + 2 e^{-}$

Suggest Corrections

Similar questions

C u + H N O_{3} \to C u (N O_{3})_{2} + N O_{2} + H_{2} O

N O_{3}^{-}

N O

N O_{2}

H N O_{3}

[C u^{2 +}] = 0.1 M

P_{N O} = P_{N O_{2}} = 10^{- 3}

H N O_{3}

N O_{3}^{-}

N O

N O_{2}

E_{C u^{2 +} | C u}^{\circ} = + 0.34 V, E_{N O_{3}^{-} | N O}^{\circ} = + 0.96 V, E_{N O_{3}^{-} | N O_{2}}^{\circ} = + .79 V

C u + N O_{3}^{-} + . . . . \to C u^{2 +} + N O_{2} + . . . . .

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 +}

{H g}^{2 +} + {N O}_{2}^{-} + H_{2} O ⟶ H g + {N O}_{3}^{-} + 2 H^{+}

Join BYJU'S Learning Program