Given a reaction:
$4 N H_{3} (g) + 5 O_{2} (g) \to 4 N O (g) + 6 H_{2} O (g)$
When $1$ mole of ammonia and $1$ mole of $O_{2}$ are made to react to completion :

1.0

mole of

H_{2} O

is produced

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1.0

mole of

N O

will be produced

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all the oxygen will be consumed

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all the ammonia will be consumed

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Solution

The correct option is C all the oxygen will be consumed
4 moles of ammonia react with 5 moles of oxygen as per the balanced chemical equation. When 1 mole of ammonia is present, it will react with 1.25 moles of oxygen. However, only 1 mole of oxygen is present.

Hence, oxygen is the limiting reagent and is completely consumed during the reaction.

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Similar questions

4 N H_{3} (g) + 5 O_{2} (g) \to 4 N O (g) + 6 H_{2} O (l)

O_{2}

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

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

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

2 S O_{2} (g) + O_{2} (g) \to 2 S O_{3} (g),

S O_{2}

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