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Balancing Red...

Balancing Redox Equations

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Q.

In the balanced chemical reaction,
$I O_{3}^{-} + a I^{-} + b H^{+} ⟶ c H_{2} O + d I_{2}$
a, b, c and d respectively correspond to

5, 6, 3, 3
5, 3, 6, 3
3, 5, 3, 6
5, 6, 5, 5

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Q.

C_{2} H_{6} (g) + n O_{2} \to C O_{2} (g) + H_{2} O (I)

In this equation, the ratio of the coefficients of

C O_{2}

and

H_{2} O

is

1 : 1
2 : 3
3 : 2
1 : 3

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Q. Oxidation of thiosulphate

(S_{2} O_{3}^{2 -})

ion by iodine gives

$S O_{3}^{2 -}$
$S O_{4}^{2 -}$
$S_{4} O_{6}^{2 -}$
$S_{2} O_{6}^{2 -}$

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Q. Balance the following redox reactions by ion-electron method.

H_{2} O_{2} (a q) + F e^{2 +} (a q) \to F e^{3 +} (a q) + H_{2} O (l)

(in acidic solution)

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Q. Balance the following redox reactions by the ion-electron method in basis medium

M n O_{4}^{-} (a q) + I^{-} (a q) \to M n O_{2} (s) + I_{2} (s)

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Q. Balance the following redox reactions by the ion-electron method in acidic medium.

M n O_{4}^{-} (a q) + S O_{2} (g) \to M n^{2 +} (a q) + H S O_{4}^{-} (a q)

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Q. For decolourization of 1 mole of

K M n O_{4}

, the moles of

H_{2} O_{2}

required is

$\frac{1}{2}$
$\frac{3}{2}$
$\frac{5}{2}$
$\frac{7}{2}$

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Q. If ten volumes of dihydrogen gas reacts with five volumes of dioxygen gas, how many volumes of water vapour would be produced?

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Q. Complete the following chemical reactions. Classify the below into (a) hydrolysis, (b) redox and (c) hydration reactions.

(i)

P b S (s) + H_{2} O_{2} (a q) \to

(ii)

M n O_{4}^{-} (a q) + H_{2} O_{2} (a q) \to

(iii)

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

(iv)

A l C l_{3} (g) + H_{2} O (l) \to

(v)

C a_{3} N_{2} (s) + H_{2} O (l) \to

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Q. Rationalise the given statements and give chemical reactions.
(a) Lead(II) chloride reacts with

C l_{2}

to give

P b C l_{4}

.
(b) Lead(IV) chloride is highly unstable towards heat.
(c) Lead is known not to form an iodide,

P b I_{4}

.

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Q.

when $S O_{2}$ is passed in a solution of potassium iodate, the oxidation state of iodine change's from :

+5 to 0
-5 to 0
-7 to -1
+5 to -1

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Q.

Oxidation number of carbon in $C_{3} O_{2}$ , $M g_{2} C_{3}$ , are respectively

-4/3, +4/3
+4/3, -4/3
-2/3, +2/3
-2/3, +4/3

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Q.

In the redox reaction

xMnO +y $P b O_{2}$ +z $H N O_{3}$ $⟶$ $H M n O_{4}$ + $P b (N O_{3})_{2}$ + $H_{2} O$

X = 2, Y =5, Z= 10
x =2, y = 7, z=8
x= 2, y =5 , z=8
x=2, y =5 , z=5

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Q. Complete the following chemical reaction and classify the into (a) hydrolysis, (b) redox and (c) hydration reactions.

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

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Q.

Consider the following reaction

$x M n O_{4}^{-} + y C_{2} O_{4}^{2 -} + z H^{+} ⟶ M n^{+ 2} + 2 y C O_{2} + \frac{z}{2} H_{2} O$

the values of x, y and z in the reaction are, respectively:

2, 5 and 16
5, 2 and 8
5, 2 and 16
2, 5 and 8

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Q. In the reaction

I_{2} + 2 S_{2} O_{3}^{- -} \to 2 I^{-} + S_{4} O_{6}^{- -}

equivalent weight of iodine will be equal to

$\frac{1}{2}$ of molecular weight
Molecular weight
$\frac{1}{4}$ of molecular weight
None

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Q. What are the two different oxidation states of carbon in Carbon suboxide

(C_{3} O_{2})

?

$+ 2, 0$
$+ 4, 0$
$+ 2, - 2$
None of the above

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Q. State as to why:
(a) a solution of

N a_{2} C O_{3}

is alkaline ?
(b) alkali metals are prepared by electrolysis of their fused chlorides ?
(c) sodium is found to be more useful than potassium ?

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Q. For the redox reaction,

M n O_{4}^{-} + C_{2} O_{4}^{2 -} + H^{+} \to M n^{2} + C O_{2} + H_{2} O

The correct coefficients of the reactants for the balanced equation are:

$M n O_{4}^{-}$ - 2, $C_{2} O_{4}^{2 -}$ - 16, $H^{+}$ - 5
$M n O_{4}^{-}$ - 2, $C_{2} O_{4}^{2 -}$ - 5, $H^{+}$ - 16
$M n O_{4}^{-}$ - 16, $C_{2} O_{4}^{2 -}$ - 5, $H^{+}$ - 2
$M n O_{4}^{-}$ - 5, $C_{2} O_{4}^{2 -}$ - 16, $H^{+}$ - 2

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Q. Which one of the following electrolytes has the same value of van't Hoff factor

(i)

as that of

K_{4} F e (C N)_{6}

(if all are 100% ionised)?

$N a_{2} S O_{4}$
$A l (N O_{3})_{3}$
$N a C l$
$A l_{2} (S O_{4})_{3}$

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Q. Water is added in excess to a

100 g

sample labelled as

112 %

H_{2} S O_{4}

This solution is then treated with

5.3 g

of

N a_{2} C O_{3}

. the volume of

C O_{2}

evolved at 1atm and

300 K

after a complete reaction will be :

H_{2} S O_{4} + N a_{2} C O_{3} \to N a_{2} S O_{4} + H_{2} O + C O_{2}

2.46 L
24.60 L
1.27 L
12.30 L

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Q. Consider the following reaction:

x M n O_{4}^{-} + y C_{2} O_{4}^{2 -} + z H^{+} \to x M n^{2 +} + 2 y C O_{2} + \frac{z}{2} H_{2} O

The values of x, y and z in the reaction are, respectively:

5, 2 and 16
2, 5 and 8
2, 5 and 16
5, 2 and 8

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Q.

X $H_{2} S O_{4}$ +Y $S O_{2}$ +Z $N a_{2} C r o_{4}$ $⟶$ $C r_{2} (S O_{4})_{3}$ ) +A $N a_{2} S O_{4}$ +B $H_{2} O$ X, Y, Z, AandB are?

2, 3, 2, 2, 2
2, 2, 2, 2, 2
4, 3, 2, 1, 0
0, 1, 2, 3, 4

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Q. For the redox reaction

M n O_{4}^{-} + C_{2} O_{4}^{- 2} + H^{+} \to M n^{2 +} + C O_{2} + H_{2} O

the correct coefficients of the reactants for the balanced reaction are

$\begin{matrix} M n O_{4}^{-} & C_{2} O_{4}^{2 -} & H^{+} 2 & 5 & 16 \end{matrix}$
$\begin{matrix} M n O_{4}^{-} & C_{2} O_{4}^{2 -} & H^{+} 16 & 5 & 2 \end{matrix}$
$\begin{matrix} M n O_{4}^{-} & C_{2} O_{4}^{2 -} & H^{+} 5 & 16 & 2 \end{matrix}$
$\begin{matrix} M n O_{4}^{-} & C_{2} O_{4}^{2 -} & H^{+} 2 & 16 & 5 \end{matrix}$

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Q.

H_{2} O_{2} + 2 K I 40 % yield - ---- \to I_{2} + 2 K O H

H_{2} O_{2} + 2 K M n O_{4} + 3 H_{2} S O_{4} 50 % yield - ---- \to K_{2} S O_{4} + 2 M n S O_{4} + 3 O_{2} + 4 H_{2} O

150 mL

of

H_{2} O_{2}

sample was divided into two parts. The first part was treated with

K I

and the formed

K O H

required

200 mL

of

M / 2

H_{2} S O_{4}

for neurtralisation. The other part was treated with

K M n O 4

, which yielded 6.74 litre of

O_{2}

at 1 atm and

273 K

. Using the percentage yield indicated, find the volume strength of the

H_{2} O_{2}

sample used.

5.04
10.08
3.36
33.6

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Q. For the reaction between

K M n O_{4}

and

H_{2} O_{2}

, the number of electrons transferred per mole of

H_{2} O_{2}

is:

One
Two
Three
Four

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Q. Write fully balanced equations for the following:

N a_{2} O + H_{2} O \to

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Q. 25 ml solution has

[C_{2} O_{4}]^{2 -}

ions. It is found to require 10 ml of

\frac{N}{10}

acidic

K_{2} C r_{2} O_{7}

for a complete reaction. Find out the molarity of

[C_{2} O_{4}]^{2 -}

in the solution.

$\frac{1}{25}$
$\frac{1}{10}$
$\frac{1}{20}$
$\frac{1}{50}$

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