To determine the number of moles of [tex]\( \text{NO} \)[/tex] formed from 2.58 moles of [tex]\( \text{NO}_2 \)[/tex] given the balanced chemical reaction:
[tex]\[
3 \, \text{NO}_2(g) + \text{H}_2\text{O}(l) \rightarrow 2 \, \text{HNO}_3(aq) + \text{NO}(g)
\][/tex]
follow these steps:
1. Identify the stoichiometric coefficients:
- From the balanced reaction, 3 moles of [tex]\( \text{NO}_2 \)[/tex] produce 1 mole of [tex]\( \text{NO} \)[/tex].
2. Write the mole ratio:
- The ratio of moles of [tex]\( \text{NO} \)[/tex] to moles of [tex]\( \text{NO}_2 \)[/tex] is [tex]\( \frac{1 \text{ mole NO}}{3 \text{ moles NO}_2} \)[/tex].
3. Calculate the moles of [tex]\( \text{NO} \)[/tex] produced:
- Using the mole ratio, you can find the moles of [tex]\( \text{NO} \)[/tex] produced from 2.58 moles of [tex]\( \text{NO}_2 \)[/tex].
[tex]\[
\text{moles of NO} = 2.58 \, \text{moles of} \, \text{NO}_2 \times \frac{1 \text{ mole of NO}}{3 \text{ moles of} \, \text{NO}_2}
\][/tex]
4. Perform the multiplication:
- Calculate the result:
[tex]\[
\text{moles of NO} = 2.58 \times \frac{1}{3}
\][/tex]
Therefore, the number of moles of [tex]\( \text{NO} \)[/tex] produced is [tex]\( 0.86 \)[/tex] moles.
So, from 2.58 moles of [tex]\( \text{NO}_2 \)[/tex] with plenty of water present, 0.86 moles of [tex]\( \text{NO} \)[/tex] will be formed.
