Balancing Red...

Balancing Redox Equations

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Q. For the reaction,

I^{-} + C l O_{3}^{-} + H_{2} S O_{4} \to C l^{-} + H S O_{4}^{-} + I_{2}

the correct statement (s) in the balanced equation is/are.

stoichiometric coefficient of $H S O_{4}^{-}$ is 6
Iodide is oxidised
Sulphur is reduced
$H_{2} O$ is one of the products

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Q. A sample of hard water contains

96 ppm

S O 4_{4}^{2 -}

ions,

183 ppm

H C O_{3}^{-}

ions and the only cation present is

C a^{2 +}

X

moles of

C a O

are required to remove the

H C O_{3}^{-}

ions from

1000 kg

of this sample of water. When the same amount of

C a O

is added to the water sample, the concentration of residual

C a^{2 +}

ions (in ppm) becomes Y.
(Assume

C a C O_{3}

to be completely insoluble in water)
If the residual

C a^{2 +}

ions in

1 L

of the above -mentioned water sample is completely replaced by hydrogen ions, what will the

p H

of the resultant sample of hard water?

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The number of atoms of each element remains the same before and after a chemical reaction.

True
False

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What do you understand by the term simple radical?

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Q. In the reaction

x H I + y H N O_{3} \to N O + I_{2} + H_{2} O

x = 1, y = 5
x = 2, y = 10
x = 6, y = 2
x = 6, y = 1

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Q. In a balanced equation

H_{2} S O_{4} + x H I \to H_{2} S + y I_{2} + z H_{2} O

, the values of x, y, z are

x = 3, y = 5, z = 2
x = 4, y = 8, z = 5
x = 8, y = 4, z = 4
x = 5, y = 3, z = 4

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2.68 \times 10^{- 3}

moles of a solution containing an ion

A^{n +}

require

1.61 \times 10^{- 3}

moles of

M n O_{4}^{-}

for the oxidation of

A^{n +}

A O_{3}^{-}

in acidic medium. What is the value of

n

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Q. Consider the reaction,

a F e S_{2} + b O_{2} \to c F e_{2} O_{3} + d S O_{2}

Which of the following options are incorrect for the above reaction?

N- factor of $F e S_{2}$ is 11
The ratio of moles of a : b is 4 : 11
The ratio of moles of a : b is 11 : 4
The ratio of moles of c : d is 1 : 4

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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. In the ionic equation for the reaction:

I O_{3}^{-} + H^{+} + a e^{-} \to I^{-} + H_{2} O

the value of 'a' is

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Q. Consider a titration of potassium dichromate solution with acidified Mohr's salt solution using diphenylamine as indicator. the number of moles of Mohr's salt required per mole of dichromate is

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Q. What is the equivalent mass of

I O_{4}^{-}

when it is converted into

I_{2}

in acid medium

$\frac{M}{6}$
$\frac{M}{7}$
$\frac{M}{5}$
$\frac{M}{4}$
None of these

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The number of electrons involved in the reduction of $C r_{2} O_{7}^{2 -}$ in acidic solution to $C r^{3 +}$ is

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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

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

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. The equivalent weight of

K I O_{3}

in the reaction

2 C r (O H)_{3} + 4 O H + K I O_{3} \to 2 C r O_{4}^{2 -} + 5 H_{2} O + K I

Mole wt.
$\frac{M o l . w t .}{6}$
$\frac{M o l . w t .}{2}$
$\frac{M o l . w t .}{3}$

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Q. The equivalent weight of

K I O_{3}

in the reaction

2 C r (O H)_{3} + 4 O H + K I O_{3} \to 2 C r O_{4}^{2 -} + 5 H_{2} O + K I

Mole wt.
$\frac{M o l . w t .}{6}$
$\frac{M o l . w t .}{2}$
$\frac{M o l . w t .}{3}$

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Q. Consider the disproportionation of Iodine to iodide and iodate ions. Using Oxidation method calculate the ratio of iodate and iodide ions formed in alkaline medium :

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

$5 : 1$
$1 : 5$
$3 : 1$
$1 : 3$

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Q. Consider the reaction,

a F e S_{2} + b O_{2} \to c F e_{2} O_{3} + d S O_{2}

Which of the following options are incorrect for the above reaction?

N- factor of $F e S_{2}$ is 11
The ratio of moles of a : b is 4 : 11
The ratio of moles of a : b is 11 : 4
The ratio of moles of c : d is 1 : 4

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Q. In the balanced chemical reaction

I O_{3}^{-} + a I^{-} + b H^{+} \to 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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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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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. 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. In the following reaction:

P_{4} (s) + O H^{-} (a q) \to P H_{3} (g) + H_{2} P O_{2}^{-} (a q)

Calculate the stoichiometric coefficient of

O H^{-}

and

H_{2} O

respectively present in a balanced equation in a basic medium?

$3 H_{2} O, 3 O H^{-}$
$6 H_{2} O, 6 O H^{-}$
$3 H_{2} O, 6 O H^{-}$
$6 H_{2} O, 3 O H^{-}$

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Q. A sample of hard water contains

96 ppm

S O 4_{4}^{2 -}

ions,

183 ppm

H C O_{3}^{-}

ions and the only cation present is

C a^{2 +}

X

moles of

C a O

are required to remove the

H C O_{3}^{-}

ions from

1000 kg

of this sample of water. When the same amount of

C a O

is added to the water sample, the concentration of residual

C a^{2 +}

ions (in ppm) becomes Y.
(Assume

C a C O_{3}

to be completely insoluble in water)
If the residual

C a^{2 +}

ions in

1 L

of the above -mentioned water sample is completely replaced by hydrogen ions, what will the

p H

of the resultant sample of hard water?

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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. 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. 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. Calculate the maximum amount of

B a_{3} (P O_{4})_{2}

that will form by the reaction of 1 mol of

B a C l_{2}

with 0.4 mol of

N a_{3} P O_{4}

0.8 mol
0.5 mol
0.2 mol
1 mol

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Q. For the redox reaction

x P_{4} + y H N O_{3} \to H_{3} P O_{4} + N O_{2} + H_{2} O

x = 1, y = 5
x = 2, y = 10
x = 1, y = 20
x = 1, y = 15

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For the redox reaction
$M n O_{4}^{-} + C_{2} O_{4}^{- 2} + H^{+} ⟶ M n^{2 +} + C O_{2} + H_{2} O$
the correct coefficients of the reactants $M n O_{4}^{-}, C_{2} O_{4}^{2 -} a n d H^{+}$ for the balanced reaction are

2, 5, 16
16, 5, 2
5, 16, 2
2, 16, 5

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