Dinitrogen monoxide (nitrous oxide) reacts with oxygen gas according to the unbalanced equation given below:
$N_{2} O (g) +$ $O_{2} (g) \to$ $N O_{2} (g)$
From the reaction mixture shown in the figure, answer the question that follows.
If the reaction mixture is ignited by a spark, and assuming that it goes to completion, which of the statements below describes the final composition of the system?

8

molecules of nitrogen dioxide are produced. Two molecules of each reactant remain.

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8

molecules of nitrogen dioxide are produced. Oxygen gas is the limiting reactant and is totally consumed.

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8

molecules of nitrogen dioxide are produced. Nitrous oxide is the limiting reactant and is totally consumed.

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12

molecules of nitrogen dioxide are produced. Nitrous oxide is the limiting reactant and is totally consumed.

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Solution

The correct option is A $8$ molecules of nitrogen dioxide are produced. Two molecules of each reactant remain.

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Similar questions

N_{2} O (g) +

O_{2} (g) \to

N O_{2} (g)

A_{2}

B_{2}

2 A_{2} + B_{2} \to 2 A_{2} B

A_{2} B

N O

20.3 g

5.89 g

Gases evolved during the thermal decomposition of mercuric nitrate $H g (N O_{3})_{2}$ are:

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