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1

### AIPMT 2008

Number of moles of MnO$$_4^{ - }$$ required to oxidize one mole of ferrous oxalate completely in acidic medium will be
A
7.5 moles
B
0.2 moles
C
0.6 moles
D
0.4 moles

## Explanation

The balanced ionic equation for oxidation of ferrous oxalate by MnO4 in acidic medium is as follows :

3MnO4- + 5FeC2O4 + 24H+ $$\to$$

3Mn2+ + 10CO2 + 12H2O + 5Fe3+

Thus, 5 moles of FeC2O4 require 3 moles of MnO4-.

So, 1 mole of FeC2O4 requires

= $${3 \over 5}$$ = 0.6 moles of MnO4-
2

### AIPMT 2004

Which is the best description of the behaviour of bromine in the reaction given below?
H2O + Br2 $$\to$$ HOBr + HBr
A
Proton acceptor only
B
Both oxidised and reduced
C
Oxidised only
D
Reduced only

## Explanation

H2O + $${\mathop {Br}\limits^0}$$2 $$\to$$ HO$$\mathop {Br}\limits^{ + 1}$$ + H$$\mathop {Br}\limits^{ - 1}$$

In the above reaction the oxidation number of Br2 increases from zero (in Br2 ) to +1 (in HOBr) and decreases from zero (in Br2 ) to –1 (in HBr). Thus Br2 is oxidised as well as reduced and hence it is a redox reaction.
3

### AIPMT 2003

The oxidation states of sulphur in the anions

SO3$${_3^{2 - }}$$, S2O$${_4^{2 - }}$$ and S2O$${_6^{2 - }}$$ follow the order
A
S2O$${_4^{2 - }}$$ < SO$${_3^{2 - }}$$ < S2O$${_6^{2 - }}$$
B
SO$${_3^{2 - }}$$ < S2O$${_4^{2 - }}$$ < S2O$${_6^{2 - }}$$
C
S2O$${_4^{2 - }}$$ < S2O$${_6^{2 - }}$$ < SO$${_3^{2 - }}$$
D
S2O$${_6^{2 - }}$$ < S2O$${_4^{2 - }}$$ < SO$${_3^{2 - }}$$

## Explanation

SO32– : oxidation state of ‘S’ is +4

S2O42– : oxidation state of ‘S’ is +3.

S2O62– : oxidation state of ‘S’ is +5.

So, the order is S2O$${_4^{2 - }}$$ < SO$${_3^{2 - }}$$ < S2O$${_6^{2 - }}$$.

#### Questions Asked from Redox Reactions

On those following papers in MCQ (Single Correct Answer)
Number in Brackets after Paper Indicates No. of Questions
NEET 2020 Phase 1 (1)
NEET 2019 (1)
NEET 2018 (3)
NEET 2016 Phase 2 (1)
AIPMT 2014 (3)
AIPMT 2012 Prelims (2)
AIPMT 2009 (1)
AIPMT 2008 (1)
AIPMT 2004 (1)
AIPMT 2003 (1)

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