Water gas is an equi-molar mixture of hydrogen and carbon monoxide. If 250 litres of water gas is burnt in air. Assuming both reactants and products are at same temperature and pressure, the volume of $O_{2}$ required is _________.
$2 C O + O_{2} \to 2 C O_{2}; 2 H_{2} + O_{2} \to 2 H_{2} O$

250 litres

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125 litres

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75 litres

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500 litres

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Solution

The correct option is B 125 litres
Equation for combustion of water gas in air is:

$2 C O + O_{2} \to 2 C O_{2}$ & $2 H_{2} + O_{2} \to 2 H_{2} O$

For combustion of $1$ mole of water gas ( $C O + H_{2}$ ) , $1 / 2$ mole of $O_{2}$ is required.

Therefore, for combustion of $250 L$ of water gas, amount of oxygen required $= \frac{250}{2} = 125 L$ of $O_{2}$ is required.

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Similar questions

C O_{2}

2 C O + O_{2} \to 2 C O_{2};

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

2 C O + O_{2} \to 2 C O_{2}

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

2 C O + O_{2} \to 2 C O_{2}

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

2 C O + O_{2} \to 2 C O_{2}

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

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?

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