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Redox Reactions
Question
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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) + 2 Cu2+ (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)

 

Answer

a)    AgBr is reduced to Ag

C6H6O2 is oxidised to C6H4O2

AgBr is an oxidising agent

C6H6O2 is a reducing agent.

b)    [Ag(NH3)+2 reduced to Ag+

HCHO is oxidised to HCOO-

[Ag(NH3)+2 is an oxidising agent.

c)   HCHO is oxidised to HCOO-

Cu2+ is reduced to Cu(I)  state.

d)   N2H4 is reduced to H2O

H2O2 is an oxidising agent

N2H4 is reducing agent.

 

e)  Pb has been oxidised to PbSO4

PbO2 is reduced to PbSO4

PbO2 is an oxidising agent

Pb is a reducing agent.

 

 

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Some More Questions From Redox Reactions Chapter

Can oxidation occur without reduction?

What are redox reactions?

What are direct redox reactions? Give one example.

What are indirect redox reactions?

Write formulas for the following compounds:
(a) Mercury (II) chloride
(b) Nickel (II) sulphate
(c) Tin (IV) oxide
(d) Thallium (I) sulphate
(e) Iron (III) sulphate
(f) Chromium (III) oxide

What are electrolytes?

What are cations and anions?

What is electrolysis?