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Introduction ...

Introduction to Oxidation and Reduction

Trending Questions

Q.

Write the complete balanced reaction (a) Potassium bromide(aq) + Barium iodide(aq) → Potassium iodide(aq) + Barium bromide(s)

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Q.

What happens when Magnesium burns in air? Write a balanced equation.

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Q.

What does the given reaction indicate? $Cu + 2 {AgNO}_{3} \to Cu {({NO}_{3})}_{2} + 2 Ag$

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Q. 1 molal aqueous solution of an electrolyte

A_{2} B_{3}

is 60% ionised . The boiling point of the solution at 1 atm in K is ( Rounded -off to the nearest integer )

[K_{b} f o r (H_{2} O) = 0.53 K K g m o l^{- 1}]

(JEE MAIN 2021)

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Q. The indicator used in the titration of iodine against sodium thiosulphate is:

Starch
$K_{3} F e (C N)_{6}$
$K_{2} C r O_{4}$
Potassium

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Q. Oxidation number of cobalt in

[C o (N H_{3})_{6}] C l_{2} B r

is -

6
3
zero
2

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Q.

“Oxidation and reduction process occurs simultaneously”. Justify the statement with the help of an example.

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Q.

$H_{2} O_{2}$ is: ?

an oxidising agent
a reducing agent
both oxidising and reducing agent
None of these

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Q. The percentage of free

S O_{3}

in an oleum is

60 %

. The given sample in terms of

% H_{2} S O_{4}

can be labelled as :

$160 %$
$140 %$
$113.5 %$
$104.5 %$

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Q. The volume strength of

8.9 M H_{2} O_{2}

solution calculated at

273 K

and

1 a t m

is _____. (

R = 0.0821 L a t m K^{- 1} m o l^{- 1}

) (rounded off to the nearest integer)

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Q.

Which of the following is not an example of redox reaction?
(a) $C u O + H_{2} \to C u + H_{2} O$
(b) $F e_{2} O_{3} + 3 C O \to 2 F e + 3 C O_{2}$
(c) $2 K + F_{2} \to 2 K F$
(d) $B a C l_{2} + H_{2} S O_{4} \to B a S O_{4} + 2 H C l$

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Q.

The percentage of available chlorine in a pure bleaching powder $(Ca {(OCl)}_{2})$ sample is ______

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Q. Which of the following is not oxidation?

Removal of Hydrogen
Addition of Electronegative element
Removal of Electropositive element
Addition of Electropositive element

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Q.

What is a redox reaction with an example?

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Q.

The reaction $4 {NH}_{3} + 5 O_{2} \to 4 NO + 6 H_{2} O$ is an example of I. Combination II. Displacement III. Redox IV, Neutralisation.

I and II
I and III
II and III
I and IV

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Q.

K_{2} M n O_{4}

in acidic or neutral medium undergo disproportionation reaction to give

$M n O_{4}^{-}$
$M n O_{2}$
$M n O_{4}^{2 -}$
$M n_{2} O_{4}^{2 -}$

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Q.

When an oxide of a non-metal reacts with water, which of the following is formed?

Acid
Base
Salt
None of these

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Q.

4.5 g

water is added into an oleum sample labelled as

109 % H_{2} S O_{4} .

What is the amount of free

S O_{3}

remaining in the solution?

$10 g$
$12 g$
$20 g$
$24 g$

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Q.

A sample of $A g C l$ was treated with $500 m L$ of $1.5 M$ $N a_{2} C O_{3}$ solution to give $A g_{2} C O_{3}$ . The remaining solution contained $0.0026 g$ of $C l^{-}$ per litre. The solubility product of $A g C l$ is if $K_{s p} (A g_{2} C O_{3}) = 8.2 \times 10^{- 12}$

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Q.

Name the process of conversion of $K_{2} {Cr}_{2} O_{7}$ into $C r_{2} {(S O_{4})}_{3}$ .

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Q. What is the

%

of free

S O_{3}

in an oleum that is labelled as

104.5 % H_{2} S O_{4}

?

10
20
40
50

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Q. When

K M n O_{4}

is reduced with oxalic acid in acidic solution, the change in oxidation number of

M n

is

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Q.

Dichromate ion is treated with base, the oxidation number of $Cr$ in the product formed in the following reaction is:

${Cr}_{2} O_{7}^{- 2} + 2 {OH}^{-} ⇌ 2 {CrO}_{4}^{- 2} + H_{2} O$

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Q. When

N a_{2} S_{2} O_{3}

reacts with

I_{2}

to form

N a_{2} S_{4} O_{6}

and

N a I

then which statement(s) is correct?

n-factor for $N a_{2} S_{2} O_{3}$ is one
n-factor for $I_{2}$ is two
2 moles of $N a_{2} S_{2} O_{3}$ is reacted with 1 mole of $I_{2}$
n-factor for $N a_{2} S_{4} O_{6}$ is one

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Q. In an aqueous solution of barium nitrate, the

[N O_{3}^{-}]

is 0.080 M. This solution can be labeled as

$0.040 N (B a (N O_{2})_{2}$
$0.160 M B a (N O_{3})_{2}$
$0.080 N B a (N O_{3})_{2}$
$0.080 M N O_{3}^{-}$

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Q. On heating, a sample of

N a C l O_{3}

, it gets converted to

N a C l

with a loss of 0.16 g of oxygen. The residue is dissolved in water and precipitated as

A g C l

. The mass of

A g C l

(in g) obtained will be :
(Given molar mass of

A g C l = 143.5 g m o l^{- 1}

)

$0.35$
$0.54$
$0.41$
$0.48$

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Q.

2 N H C l

solution will have the same molar concentration as:

$4.0 N H_{2} S O_{4}$
$0.5 N H_{2} S O_{4}$
$1 N H_{2} S O_{4}$
$2 N H_{2} S O_{4}$

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Q.

Explain by giving one example why do oxidation and reduction proceed side by side ?

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Q.

Calculate the percentage of iron in K₃Fe(CN)₆ (K = 39, Fe = 56, C = 12, N = 14).

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Q.

For a redox reaction to proceed in a cell, the e.m.f. must be:

Fixed
Zero
Positive
Negative

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