Water-gas is an equimolar mixture of hydrogen and carbon monoxide. If 250 litres of water gas is burnt in air. Assuming both reactants and products are at the same temperature and pressure, the volume of $C O_{2}$ produced is:

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

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

125 litres

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62.5 litres

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250 litres

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500 litres

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Solution

The correct option is D 125 litres
$2 C O + O_{2} = 2 C O_{2};$

$2 H_{2} + O_{2} = 2 H_{2} O$

Given, $C O + H_{2} = 250 L$

Since $C O$ and $H_{2}$ are equimolar, so each has vol 125 L (Given total volume is 250 L.)

The equation shows that :

2 L of $C O$ gives 2 L of $C O_{2}$

So, 125 L of $C O$ gives 125 L of $C O_{2}$

Hence, option (a) is correct.

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Similar questions

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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