Which equation is correctly labeled oxidation or reduction?

H_{2} S = S + 2 e^{-} + 2 H^{+}

oxidation

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S O_{2} + 4 e^{-} + 2 H_{2} O = S + 4 O H^{-}

oxidation

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N H_{3} + H C l = N H_{4} + + {C l}_{2}^{-}

oxidation

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N a C l + A g N O_{3} = A g C l + N a N O_{3}

reduction

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M n^{2 +} = M n O_{4}^{-}

reduction

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Solution

The correct option is A $H_{2} S = S + 2 e^{-} + 2 H^{+}$
oxidation
The equation of the option A, $H_{2} S = S + 2 e^{-} + 2 H^{+}$ is correctly labeled oxidation.
The loss of electrons is oxidation whereas gain of electrons is the reduction.

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Similar questions

Given :

Oxidation :

$H_{2} O_{2} \to O_{2} + 2 H^{\oplus} + 2 e^{-}$

$E^{⊖} = - 0.69 V$ ;

$2 F^{⊖} \to F_{2} + 2 e^{-}$

$E^{⊖} = - 2.87 V$ ;

Reduction :

$H_{2} O_{2} + 2 H^{\oplus} + 2 e^{-} \to 2 H_{2} O$

$E^{⊖} = - 1.77 V$ ;

$2 I^{⊖} \to I_{2} + 2 e^{-}$ $E^{⊖} = - 0.54 V$ ;

Which of the following statements is/are correct ?

Find out the process of oxidation , reduction. And oxidising agent ,reducing agent from the following.

1. MnO₂ + 4HCL ➡ MnCl₂ + 2H₂O + Cl₂

2.H₂S + SO₂➡ S+ H₂O

3.CuO + C ➡ Cu + CO

Q. Rank the following elements by increasing ease of oxidation with most easily oxidized LAST:

C d, C u, N i, F e

Standard Reduction Potentials at

25^{\circ} C

Half-Reaction	$E^{\circ} (V)$
$F_{2} + 2 e^{-} \to 2 F^{-}$	$2.87$
$A g^{2} + e^{-} \to A g^{+}$	$1.99$
$C o^{3 +} + e^{-} \to C o^{2 +}$	$1.82$
$H_{2} O_{2} + 2 H^{+} + 2 e^{-} \to 2 H_{2} O$	$1.78$
$M n O_{4}^{-} + 4 H^{+} + 3 e^{-} \to M n O_{2} + 2 H_{2} O$	$1.68$
$2 e^{-} + 2 H^{+} + I O_{4}^{-} \to I O_{3}^{-} + H_{2} O$	$1.60$
$M n O_{4}^{-} + 8 H^{+} + 5 e^{-} \to M n^{2 +} + 4 H_{2} O$	$1.51$
$A u^{3 +} + 3 e^{-} \to A u$	$1.50$
$C l_{2} + 2 e^{-} \to 2 C l^{-}$	$1.36$
$O_{2} + 4 H^{+} + 4 e^{-} \to 2 H_{2} O$	$1.23$
$M n O_{2} + 4 H^{+} + 2 e^{-} \to M n^{2 +} + 2 H_{2} O$	$1.21$
$B r_{2} + 2 e^{-} \to 2 B r^{-}$	$1.09$
$N O_{3}^{-} + 4 H^{+} + 3 e^{-} \to N O + 2 H_{2} O$	$0.96$
$C l O_{2} + e^{-} \to C l O_{2}$	$0.954$
$2 H g^{2 +} + 2 e^{-} \to H g_{2}^{2 +}$	$0.91$
$A g^{+} + e^{-} \to A g$	$0.80$
$H g_{2}^{2 +} + 2 e^{-} \to 2 H g$	$0.80$
$F e^{3 +} + e^{-} \to F e^{2 +}$	$0.77$
$O_{2} + 2 H^{+} + 2 e^{-} \to H_{2} O_{2}$	$0.68$
$M n O_{4}^{-} + e^{-} \to M n O_{4}^{2 -}$	$0.56$
$I_{2} + 2 e^{-} \to 2 I^{-}$	$0.54$
$C u^{+} + e^{-} \to C u$	$0.52$
$O_{2} + 2 H_{2} O + 4 e^{-} \to 4 O H^{-}$	$0.40$
$C u^{2 +} + 2 e^{-} \to C u$	$0.34$
$A g C l + e^{-} \to A g + C l^{-}$	$0.22$
$C u^{2 +} + e^{-} \to C u^{+}$	$0.16$
$2 H^{+} + 2 e^{-} \to H_{2}$	$0.00$
$F e^{3 +} + 3 e^{-} \to F e$	$- 0.036$
$P b^{2 +} + 2 e^{-} \to P b$	$- 0.13$
$N i^{2 +} + 2 e^{-} \to N i$	$- 0.23$
$C d^{2 +} + 2 e^{-} \to C d$	$- 0.40$
$F e^{2 +} + 2 e^{-} \to F e$	$- 0.44$
$C r^{3 +} + e^{-} \to C r^{2 +}$	$- 0.50$
$C r^{3 +} + 3 e^{-} \to C r$	$- 0.73$
$Z n^{2 +} + 2 e^{-} \to Z n$	$- 0.76$
$2 H_{2} O + 2 e^{-} \to H_{2} + 2 O H^{-}$	$- 0.83$
$M n^{2 +} + 2 e^{-} \to M n$	$- 1.18$
$A l^{3 +} + 3 e^{-} \to A l$	$- 1.66$
$H_{2} + 2 e^{-} \to 2 H^{-}$	$- 2.23$
$M g^{2 +} + 2 e^{-} \to M g$	$- 2.37$
$N a^{+} + e^{-} \to N a$	$- 2.71$
$C a^{2 +} + 2 e^{-} \to C a$	$- 2.76$
$B a^{2 +} + 2 e^{-} \to B a$	$- 2.90$
$K^{+} + e^{-} \to K$	$- 2.92$
$L i^{+} + e^{-} \to L i$	$- 3.05$

Q. State the following is oxidation reaction or reduction reaction:

S n^{4 +} + 2 e^{-} \to S n^{2 +}

Q. State whether the following conversions are oxidation or reduction?

P b O_{2} + {S O}_{2} \to P b {S O}_{4}

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Which equation is correctly labeled oxidation or reduction?

The correct option is A H2S=S+2e−+2H+ oxidationThe equation of the option A, H2S=S+2e−+2H+ is correctly labeled oxidation.The loss of electrons is oxidation whereas gain of electrons is the reduction.

The correct option is A $H_{2} S = S + 2 e^{-} + 2 H^{+}$
oxidation
The equation of the option A, $H_{2} S = S + 2 e^{-} + 2 H^{+}$ is correctly labeled oxidation.
The loss of electrons is oxidation whereas gain of electrons is the reduction.