Question

According to the following balanced reaction, how many moles of NO are formed from 12.66 moles of NO2 if there is plenty of water present? 3 NO2(g) + H2O(l) → 2 HNO3(aq) + NO(g

Answer 1

Answer: The moles of NO produces are 4.22 moles

Step-by-step explanation:

We are given:

Moles of nitrogen dioxide = 12.66 moles

The given chemical equation follows:

`3NO_2(g)+H_2O(l)\rightarrow 2HNO_3(aq.)+NO(g)`

By Stoichiometry of the reaction:

3 moles of nitrogen dioxide produces 1 mole of NO

So, 12.66 moles of nitrogen dioxide will produce =
`(1)/(3)* 12.66=4.22mol` of NO

Hence, the moles of NO produces are 4.22 moles

Answer 2

`\boxed{\text{4.220 mol}}`

Step-by-step explanation:

3NO₂ + H₂O → 2HNO₃ + NO

n/mol: 12.66

You get 1 mol of NO from 3 mol of NO₂

`\text{Moles of NO} = \text{12.66 mol NO}_(2)* \frac{\text{1 mol NO}}{\text{3 mol NO}_(2)} = \textbf{4.220 mol NO}\\\\\text{The reaction forms } \boxed{\textbf{4.220 mol}} \text{ of NO}`