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Stoichiometric Calculations

The reaction ...

Question

The reaction between nitric oxide $(N O)$ and oxygen to form nitrogen dioxide $(N O_{2})$ is a key step in photochemical smog formation:

$2 N O (g) + O_{2} (g) ⟶ 2 N O_{2} (g)$

The grams of $N O_{2}$ formed by the reaction of 1.20 g of $N O$ is:

7.2 g

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2.3 g

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1.8 g

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4.1 g

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Solution

The correct option is C 1.8 g
$2 N O (g) + O_{2} (g) ⟶ 2 N O_{2} (g)$

2 moles of $N O$ gives 2 moles $N O_{2}$ .

Moles of NO $= \frac{1.20}{30} = 0.04$ mol

Therefore, moles of $N O_{2}$ formed $= 0.04 m o l e s = 0.04 \times 46 = 1.8$ moles

Hence, option C is correct.

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