Hydrogen sulphide gas burns in oxygen to yield 12.8 g of sulphur dioxide gas as under:
$2 H_{2} S + 3 O_{2} \to 2 H_{2} O + 2 S O_{2}$
(i). calculate the volume of hydrogen suulphide at STP.
Also, (ii). calculate the volume of oxygen required at STP. Which will complete the combustion of hydrogen sulphide determined in litres.

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Solution

The molar mass of $S O_{2}$ is 64 g/mol, it means 1 mol of $S O_{2}$ has the mass 64 grams.

At STP condition, 1 mol of gas is equal to the volume of 22.4 L. In another way, 64 g of the $S O_{2}$ is equal to 22.4 L.

Let us compare the balanced equation.

$2 H_{2} S + 3 O_{2} \to 2 H_{2} O + 2 S O_{2}$

Find the volume of $S O_{2}$

$12.8 g o f S O_{2} \times (\frac{22.4 L o f S O_{2}}{64 g S O_{2}}) = 4.48 L O_{2} g a s$

(i). Find the volume of $H_{2} S$

4.48 L of $S O_{2}$ will require = $4.48 L o f S O_{2} \times (\frac{2 L o f H_{2} S}{2 L S O_{2}}) = 4.48 L O_{2} g a s$

(ii). Find the volume of $O_{2}$ Note" Please use 4.48 L of $H_{2} S$ instead of 0.48 L of $H_{2} S$ .

4.48 L of $S O_{2}$ will require = $4.48 L o f S O_{2} \times (\frac{3 L o f O_{2}}{2 L S O_{2}}) = 6.72 L O_{2} g a s$

(iii).It is 6.72 L of $O_{2}$ to burn completely the 4.48 L of $H_{2} S$ .

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Similar questions

(a) What volume of hydrogen sulphide at STP will burn in oxygen to yield 12.8 g sulphur dioxide according to the equation?
2H₂S + 3O₂ $\overset{}{\to}$ 2H₂O + 2SO₂
(H = 1, O = 16, S = 32)
(b) For the volume of hydrogen sulphide determined in (a) above, what volume of oxygen would be required for complete combustion?

Calculate the volume of oxygen at STP required for the complete combustion of 100 litres of carbon monoxide at the same temperature and pressure.

$2 C O + O_{2} ⟶ 2 C O_{2}$

(b) $200 c m^{3}$ of hydrogen and 150 cm of oxygen are mixed and ignited, as per the following reaction,

$2 H_{2} + O_{2} ⟶ 2 H_{2} O$ . What volume of oxygen remains unreacted?

Q. At NTP, 10 litre of hydrogen sulphide gas reacted with 10 litre of sulphur dioxide gas. The volume of gas, after the reaction is complete, would be:

Q. At STP,

2.8

litres of hydrogen sulphide were mixed with

1.6

litre of sulphur dioxide and the reaction occurred according to the equation:

2 H_{2} S (g) + S O_{2} (g) \to 2 H_{2} O (l) + 3 S (s)

Which of the following shows the volume of the gas remaining after the reaction?

Q. When the gases; sulphur dioxide and hydrogen sulphide mix in the presence of water, the reaction

S O_{2} + 2 H_{2} S \to 2 H_{2} O + 3 S

occurs.
Here hydrogen sulphide is acting as :

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