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VSEPR Theory

2 litres of a...

Question

$2$ litres of an acidified solution of $K M n O_{4}$ containing $1.58$ g of $K M n O_{4}$ per litre is decolourised by passing sufficient amount of $S O_{2}$ gas. If whole of the sulphur from $x$ g of $F e S_{2}$ is converted into $S O_{2}$ to be used in above reaction. Calculate the value of $x$ .

1.5

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4.5

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Solution

The correct option is B 3
Change in an oxidation state of $M n$ is $5$ and change in the oxidation state of $S$ is $2$ .

Therefore, from the law of equivalence,

Eq. of $K M n O_{4} (v . f = 5) = E q . o f S O_{2} (v . f = 2)$

$\frac{1.58}{158} \times 5 \times 2 = n_{S O_{2}} \times 2$

$∴ n_{S O_{2}} = 0.05 m o l e s$

Whole of $S$ from $F e S_{2}$ is converted into $S O_{2}$

$t h e r e f o r e,$ Applying POAC on $S,$

$2 \times n_{F e S_{2}} = 1 \times n_{S O_{2}}$ $∴ 2 \times \frac{n_{F e S_{2}}}{120} = 1 \times 0.05$

$∴ n_{F e S_{2}} = 3 g = x$

$∴ x = 3$

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Similar questions

2

L of an acidified solution of

K M n O_{4}

containing

1.58

g of

K M n O_{4}

per litre is decolourised by passing sufficient amount of

S O_{2}

gas. If whole of the sulphur from

x

g of

F e S_{2}

is converted into

S O_{2}

to be used in the above reaction, calculate the value of

x

Q. One line of an acidified solution of

K M n O_{4}

containing

15

g of

K M n O_{4}

is decolourised by passing sufficient amount of

S O_{2}

. If

S O_{2}

is produced by roasting of iron pyrites

(F e S_{2})

and

X

g amount of pyrites is required to produce the necessary amount of

S O_{2}

, then what is the value of

X

Q. One litre of acidified

K M n O_{4}

containing 15.8 g

K M n O_{4}

(mol.wt=158) is decolourised by passing sufficient

S O_{2}

. If

S O_{2}

is produced by

F e S_{2}

, then which of the following options is/are correct?

(F e = 56, S = 32)

Q. Paragraph for below question

नीचे दिए गए प्रश्न के लिए अनुच्छेद

11.85 g KMnO₄ is dissolved in one litre of dil. H₂SO₄. To this solution, sufficient SO₂ gas is passed just to decolourise the purple colour of KMnO₄ solution.

2KMnO₄ + 5SO₂ + 2H₂O → K₂SO₄ + 2MnSO₄ + 2H₂SO₄

The SO₂ gas used in the above reaction is produced by oxidation of iron pyrites (FeS₂) as per the following reaction

4FeS₂(s) + 11O₂(g) → 2Fe₂O₃(s) + 8SO₂(g)

11.85 g KMnO₄ को एक लीटर तनु H₂SO₄ में घोला गया है। इस विलयन में, KMnO₄ विलयन के बैंगनी रंग को विरंजित करने के लिए पर्याप्त SO₂ गैस प्रवाहित की जाती है।

2KMnO₄ + 5SO₂ + 2H₂O → K₂SO₄ + 2MnSO₄ + 2H₂SO₄

उपरोक्त अभिक्रिया में प्रयुक्त SO₂ गैस को निम्नलिखित अभिक्रिया के अनुसार आयरन पाइराइट (FeS₂) के ऑक्सीकरण द्वारा प्राप्त किया जाता है।

4FeS₂(s) + 11O₂(g) → 2Fe₂O₃(s) + 8SO₂(g)

Q. Find out the volume of SO₂ gas used in the above reaction at one atm pressure and 0ºC.

प्रश्न - एक atm दाब व 0ºC पर उपरोक्त अभिक्रिया में प्रयुक्त SO₂ गैस का आयतन ज्ञात कीजिए।

Q. Paragraph for below question

नीचे दिए गए प्रश्न के लिए अनुच्छेद

11.85 g KMnO₄ is dissolved in one litre of dil. H₂SO₄. To this solution, sufficient SO₂ gas is passed just to decolourise the purple colour of KMnO₄ solution.

2KMnO₄ + 5SO₂ + 2H₂O → K₂SO₄ + 2MnSO₄ + 2H₂SO₄

The SO₂ gas used in the above reaction is produced by oxidation of iron pyrites (FeS₂) as per the following reaction

4FeS₂(s) + 11O₂(g) → 2Fe₂O₃(s) + 8SO₂(g)

11.85 g KMnO₄ को एक लीटर तनु H₂SO₄ में घोला गया है। इस विलयन में, KMnO₄ विलयन के बैंगनी रंग को विरंजित करने के लिए पर्याप्त SO₂ गैस प्रवाहित की जाती है।

2KMnO₄ + 5SO₂ + 2H₂O → K₂SO₄ + 2MnSO₄ + 2H₂SO₄

उपरोक्त अभिक्रिया में प्रयुक्त SO₂ गैस को निम्नलिखित अभिक्रिया के अनुसार आयरन पाइराइट (FeS₂) के ऑक्सीकरण द्वारा प्राप्त किया जाता है।

4FeS₂(s) + 11O₂(g) → 2Fe₂O₃(s) + 8SO₂(g)

Q. What is the minimum mass of iron pyrites required in the above reaction?

[Atomic mass in u : O = 16, S = 32, K = 39, Mn = 55, Fe = 56]

प्रश्न - उपरोक्त अभिक्रिया में आवश्यक आयरन पाइराइट का न्यूनतम द्रव्यमान क्या है?

[u में परमाणु द्रव्यमान : O = 16, S = 32, K = 39, Mn = 55, Fe = 56]

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2 litres of an acidified solution of KMnO4 containing 1.58 g of KMnO4 per litre is decolourised by passing sufficient amount of SO2 gas. If whole of the sulphur from x g of FeS2 is converted into SO2 to be used in above reaction. Calculate the value of x.

$2$ litres of an acidified solution of $K M n O_{4}$ containing $1.58$ g of $K M n O_{4}$ per litre is decolourised by passing sufficient amount of $S O_{2}$ gas. If whole of the sulphur from $x$ g of $F e S_{2}$ is converted into $S O_{2}$ to be used in above reaction. Calculate the value of $x$ .