Question

NO2 + H2O -> HNO3 + NO
How many grams of nitrogen dioxide are required in this reaction to produce 5.00 g HNO3?

Answer 1

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Answer on Question #45019 – Chemistry – Other

Question

$$\mathrm{NO_2} + \mathrm{H_2O} \rightarrow \mathrm{HNO_3} + \mathrm{NO}$$

How many grams of nitrogen dioxide are required in this reaction to produce 5.00 g HNO₃?

Solution

Molar mass of $\mathrm{NO_2}$: $\mathrm{M}(\mathrm{NO_2}) = 46.01\ \mathrm{g/mol}$

Molar mass of $\mathrm{HNO_3}$: $\mathrm{M}(\mathrm{HNO_3}) = 63.01\ \mathrm{g/mol}$

Balanced chemical equation is

$$3 \mathrm{NO_2} + \mathrm{H_2O} \rightarrow 2 \mathrm{HNO_3} + \mathrm{NO}$$

As is clear from the balanced chemical equation, 3 mol of $\mathrm{NO_2}$ are required to produce 2 mol of $\mathrm{HNO_3}$. Thus, we can write the proportion

$$2 \cdot \mathrm{M}(\mathrm{HNO_3}) - 3 \cdot \mathrm{M}(\mathrm{NO_2})$$ $$\mathrm{m}(\mathrm{HNO_3}) - \mathrm{m}(\mathrm{NO_2})$$ $$\mathrm{m}(\mathrm{NO_2}) = 3 \cdot \mathrm{M}(\mathrm{NO_2}) \cdot \mathrm{m}(\mathrm{HNO_3}) / 2 \cdot \mathrm{M}(\mathrm{HNO_3}) = 3 \cdot 46.01 \cdot 5.00 / 2 \cdot 63.0 = 5.48\ \mathrm{g}$$

Answer: 5.48 g of nitrogen dioxide are required to produce 5.00 g HNO₃