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Stoichiometric Calculations

2L of an acid...

Question

$2$ 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 $x$ .

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Solution

The oxidation reaction is as given below.
$5 S O_{2} + 2 K M n O_{4} + 2 H_{2} O \to 2 M n S O_{4} + K_{2} S O_{4} + 2 H_{2} S O_{4}$

Thus, $2$ mol $K M n O_{4}$ = 5 mol $S O_{2}$ .

The molar mass of $K M n O_{4}$ is $158 g / m o l$ .

The number of moles of $K M n O_{4}$ is $\frac{2 \times 1.58 g}{158 g / m o l} = 0.02 m o l$ .

The number of moles of $S O_{2}$ required is $0.02 m o l \times \frac{5 m o l}{2 m o l} = 0.05 m o l$ .

2 moles of $S O_{2}$ will be obtained from one mole of $F e S_{2}$ .

Hence, 0.05 moles of $S O_{2}$ will be obtained from $\frac{0.05 m o l}{2 m o l} = 0.025 m o l$ of $F e S_{2}$ .

The molar mass of $F e S_{2}$ is $120 g / m o l$ .

Hence, the mass of $F e S_{2}$ is $x = 120 g / m o l \times 0.025 m o l = 3 g$ .

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Similar questions

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

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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2L of an acidified solution of KMnO4 containing 1.58g 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 the above reaction, calculate the value of x.

$2$ 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 $x$ .