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Oxidising Reagent and Reducing Reagent

Consider the ...

Question

Consider the reactions:
(a) $H_{3} P O_{2} (a q) + 4 A g N O_{3} (a q) + 2 H_{2} O (l) \to H_{3} P O_{4} (a q) + 4 A g (s) + 4 H N O_{3} (a q)$
(b) $H_{3} P O_{2} (a q) + 2 C u S O_{4} (a q) + 2 H_{2} O (l) \to H_{3} P O_{4} (a q) + 2 C u (s) + H_{2} S O_{4} (a q)$
(c) $C_{6} H_{5} C H O (l) + 2 [A g (N H_{3}) 2]^{+} (a q) + 3 O H^{-} (a q) \to C_{6} H_{5} C O O^{-} (a q) + 2 A g (s) + 4 N H_{3} (a q) + 2 H_{2} O (l)$
(d) $C_{6} H_{5} C H O (l) + 2 C u^{2 +} (a q) + 5 O H^{-} (a q) \to$ No change observed.
What inference do you draw about the behaviour of $A g^{+} a n d C u^{2 +}$ from these reactions?

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Solution

$A g^{+}$ and $C u^{2 +}$ act as oxidising agents in reactions (a) and (b) respectively. In reaction (c), $A g^{+}$ oxidises $C_{6} H_{5} C H O$ to $C_{6} H_{5} C O O^{-}$ , but in reaction (d), $C u^{2 +}$ cannot oxidise $C_{6} H_{5} C H O .$ Hence, we can say that Ag+ is a stronger oxidising agent than $C u^{2 +}$ .

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Similar questions

Q. From the following reactions, determine if

A g^{+}

is a stronger oxidizing agent than

C u^{2 +}

H_{3} P O_{2} (a q) + 4 A g N O_{3} (a q) + 2 H_{2} O (l) \to H_{3} P O (a q) + 4 A g (s) + 4 H N O_{3} (a q)

H_{3} P O_{2} (a q) + 2 C u S O_{4} (a q) + 2 H_{2} O (l) \to H_{3} P O_{4} (a q) + 2 C u (s) + H_{2} S O_{4} (a q)

C_{6} H_{5} C H O (l) + 2 [A g (N H_{3})_{2}]^{+} (a q) + 3 O H^{-} (a q) \to C_{6} H_{5} C O O^{-} (a q)

+ 2 A g (s) + 4 N H_{3} (a q) + 2 H_{2} O (l)

C_{6} H_{5} C H O (l) + 2 C u^{2 +} (a q) + 5 O H^{-} (a q) \to

No Change observed.

Identify the substance oxidised, reduced, oxidising agent and reducing agent for each of the following reactions:

(a) 2AgBr (s) + C₆H₆O₂(aq) → 2Ag(s) + 2HBr (aq) + C₆H₄O₂(aq)

(b) HCHO(l) + 2[Ag (NH₃)₂]⁺(aq) + 3OH^–(aq) → 2Ag(s) + HCOO^–(aq) + 4NH₃(aq) + 2H₂O(l)

(c) HCHO (l) + 2Cu²⁺⁽aq) + 5 OH^–(aq) → Cu₂O(s) + HCOO^–(aq) + 3H₂O(l)

(d) N₂H₄(l) + 2H₂O₂(l) → N₂(g) + 4H₂O(l)

(e) Pb(s) + PbO₂(s) + 2H₂SO₄(aq) → 2PbSO₄(s) + 2H₂O(l)

Q. Identify the substance oxidised, reduced, oxidising agent and reducing agent for the following reaction.

{H C H O}_{(l)} + 2 [A g (N H_{3})_{2}]_{(a q)}^{+} + 3 O H_{(a q)}^{-} \to 2 A g_{(s)} + H C O O_{(a q)}^{-} + 4 {N H_{3}}_{(a q)} + 2 {H_{2} O}_{(l)}

Q. Which of the following represents the anode half-cell reaction for the following galvanic cell:

C u (s) | C u^{2 +} (a q) | | A g^{+} (a q) | A g (s)

Q. Which of the following represents the anode half-cell reaction for the following galvanic cell:

C u (s) | C u^{2 +} (a q) | | A g^{+} (a q) | A g (s)

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Oxidising Reagent and Reducing Reagent

Standard XII Chemistry

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