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Stoichiometric Calculations

A2On is oxidi...

Question

$A_{2} O_{n}$ is oxidized to $A O_{3}^{-}$ by $K M n O_{4}$ in acidic medium. If $1.34$ mmol of $A_{2} O_{n}$ requires $32.2$ ml of $0.05$ M acidified $K M n O_{4}$ solution for complete oxidation. Find the value of $n$ .

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Solution

The correct option is C $2$
Let then oxidation state of $A$ is $n$ in $A_{2} O_{n}$ .
The reaction is given below:
$A_{2} O_{n} + K M n O_{4} \to A O_{3}^{-} + M n^{+ 2}$
n +7 +5 +2

$5 - n$ factor is the number of electrons supplied/reacted per mole of the substance.
For per mole of A, the number of electrons supplied $= 5 - n$ .
As $A_{2} O_{n} \to 2 A O_{3}^{-}$ total electrons supplied $= 2 \times (5 - n)$ .

For $M n$ , number of electrons reacted $= + 7 - (+ 2) = 5$ .

So, as given
$1.34 \times 2 \times (5 - n) = 5 \times 32.2 \times 0.05$ .
or, $(5 - n) = 3$ .
or, $n = 2$ .

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Similar questions

$A_{2} O_{n}$ is oxidized to $A O_{3}^{-}$ by $K M n O_{4}$ in acidic medium. If 1.34 mmol of $A_{2} O_{n}$ requires 32.2 mL of 0.05 M acidified $K M n O_{4}$ solution for complete oxidation, which of the following statement(s) is/are correct?

1

g of

H_{2} O_{2}

solution containing

x %

H_{2} O_{2}

by mass requires

x

mL of

K M n O_{4}

for complete oxidation in acid medium. Calculate the normality of

K M n O_{4}

solution. (write the value to the nearest integer)

Q. A 3.4

g

sample of

H_{2} O_{2}

solution containing x% by mass requires

x

ml of a

K M n O_{4}

solution for complete oxidation under acidic medium. The molarity of

K M n O_{4}

solution is:

Q. A

1

g sample of

H_{2} O_{2}

containing

x

percent

H_{2} O_{2}

by weight, requires

x

mL of

K M n O_{4}

solution for complete oxidation in acidic medium. Calculate the normality of

K M n O_{4}

solution as nearest integer.

Q. The volume of

0.05 M

K M n O_{4}

solution required to oxidize completely

2.70 g

of Oxalic acid

(H_{2} C_{2} O_{4} .2 H_{2} O)

in acidic medium will be:

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A2On is oxidized to AO−3 by KMnO4 in acidic medium. If 1.34 mmol of A2On requires 32.2 ml of 0.05 M acidified KMnO4 solution for complete oxidation. Find the value of n.

$A_{2} O_{n}$ is oxidized to $A O_{3}^{-}$ by $K M n O_{4}$ in acidic medium. If $1.34$ mmol of $A_{2} O_{n}$ requires $32.2$ ml of $0.05$ M acidified $K M n O_{4}$ solution for complete oxidation. Find the value of $n$ .