From the given reactions which is a redox reaction?

C u O (s) + H_{2} (g) \to C u (s) + H_{2} O (l)

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2 C u (s) + O_{2} (g) \to 2 C u O (s)

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C (s) + 2 H_{2} (g) \to C H_{4} (g)

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4 A l (s) + 3 O_{2} (g) \to 2 A l_{2} O_{3} (s)

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Solution

The correct options are
A $C u O (s) + H_{2} (g) \to C u (s) + H_{2} O (l)$
B $2 C u (s) + O_{2} (g) \to 2 C u O (s)$
C $C (s) + 2 H_{2} (g) \to C H_{4} (g)$
D $4 A l (s) + 3 O_{2} (g) \to 2 A l_{2} O_{3} (s)$
All the given reactions are redox reactions. In these reactions, the oxidation number of both reactants changes. The oxidation number of one reactant increase and the oxidation number of other reactant decreases.

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Similar questions

C u O (s) + H_{2} (g) \to C u (s) + H_{2} O (g)

C u O (s) + H_{2} (g) \to C u (s) + H_{2} O (l)

Justify that the following reactions are redox reactions:

(a) CuO(s) + H₂(g) → Cu(s) + H₂O(g)

(b) Fe₂O₃(s) + 3CO(g) → 2Fe(s) + 3CO₂(g)

(d) 2K(s) + F₂(g) → 2K+F– (s)

(e) 4 NH₃(g) + 5 O₂(g) → 4NO(g) + 6H₂O(g)

C_{(g r a p h i t e)} + O_{2} (g) \to C O_{2} (g); Δ_{r} H^{o} = - 393.5 k J m o l^{- 1}

H_{2} (g) + \frac{1}{2} O_{2} (g) \to H_{2} O (l); Δ_{r} H^{o} = - 285.8 k J m o l^{- 1}

C O_{2} (g) + 2 H_{2} O (l) \to C H_{4} (g) + 2 O_{2} (g); Δ_{r} H^{o} = + 890.3 k J m o l^{- 1}

Δ_{r} H^{o}

298 K

C_{(g r a p h i t e)} + 2 H_{2} (g) \to C H_{4} (g)

C_{(g r a p h i t e} + O_{2} (g) \to C O_{2} (g); Δ_{r} H^{o} = - 393.5 k J m o l^{- 1}

H_{2} (g) + \frac{1}{2} O_{2} (g) \to H_{2} O (l); Δ_{r} H^{o} = - 285.8 k J m o l^{- 1}

C O_{2} (g) + 2 H_{2} O (l) \to C H_{4} (g) + 2 O_{2} (g); Δ^{r} H 6 o = + 890.3 k J m o l^{- 1}

D e l t a_{r} H^{o}

298 K

C_{(g r a p h i t e)} + 2 H_{2} (g) \to C H_{4} (g)

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