$4 N H_{3} + 5 O_{2} \to 4 N O + 6 H_{2} O$
If 27 liters of reactants are consumed, what volume of nitrogen monoxide is produced at the same temperature and pressure?

12 litres

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15 litres

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8 litres

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9 litres

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Solution

The correct option is A 12 litres
$4 N H_{3} + 5 O_{2} \to 4 N O + 6 H_{2} O$
27 litre reactants means ratio of ammonia and oxygen is 4:5.
Therefore, volume of ammonia = 12 litres, volume of oxygen = 15 litres.
12 litres of ammonia will react with 15 litres of oxygen to give 12 litres of $N O$ .

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Similar questions

(a) Concentrated nitric acid oxidises phosphorus to phosphoric acid according to the following equation:
P + 5HNO₃ $\overset{}{\to}$ H₃PO₄ + H₂O + 5NO₂
(i) What mass of phosphoric acid can be prepared from 6.2 g of phosphorus?
(ii) What mass of nitric acid will be consumed at the same time?
(iii) What will be the volume of steam at the same time measured at 760 mm Hg pressure and 373°C? (H = 1; N = 14; O = 16; P = 31)

(b) Ammonia may be oxidised to nitrogen monoxide in the presence of a catalyst according to the following equation:
4NH₃ + 5O₂ $\overset{}{\to}$ 4NO + 6H₂O
If 27 litres of reactants are consumed, what volume of nitrogen monoxide is produced at the same temperature and pressure?

The catalyst used in $4 N H_{3} + 5 O_{2} ⟶ 4 N O + 6 H_{2} O$ is___________.

Q. Unit of equilibrium constant

K_{c}

for following homogenous reaction :-

4 N H_{3} + 5 O_{2} ⇌ 4 N O + 6 H_{2} O

Q. Equivalent masses of

N H_{3}

in the reactions are :
(i)

4 N H_{3} + 5 O_{2} ⟶ 4 N O + 6 H_{2} O

(ii)

2 N H_{3} ⟶ N_{2} + 3 H_{2}

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

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4NH3+5O2→4NO+6H2OIf 27 liters of reactants are consumed, what volume of nitrogen monoxide is produced at the same temperature and pressure?

The correct option is A 12 litres4NH3+5O2→4NO+6H2O27 litre reactants means ratio of ammonia and oxygen is 4:5.Therefore, volume of ammonia = 12 litres, volume of oxygen = 15 litres.12 litres of ammonia will react with 15 litres of oxygen to give 12 litres of NO.

$4 N H_{3} + 5 O_{2} \to 4 N O + 6 H_{2} O$
If 27 liters of reactants are consumed, what volume of nitrogen monoxide is produced at the same temperature and pressure?

The correct option is A 12 litres
$4 N H_{3} + 5 O_{2} \to 4 N O + 6 H_{2} O$
27 litre reactants means ratio of ammonia and oxygen is 4:5.
Therefore, volume of ammonia = 12 litres, volume of oxygen = 15 litres.
12 litres of ammonia will react with 15 litres of oxygen to give 12 litres of $N O$ .