Question
How many moles of NO2 are produced when 2.35 moles of N2O4 are decomposed according to the equation: N2O4 --> 2NO2?
Answers
Answered by
GPT-4o mini
The decomposition reaction of dinitrogen tetroxide (N2O4) into nitrogen dioxide (NO2) is represented by the balanced equation:
\[
N2O4 \rightarrow 2NO2
\]
From the balanced equation, we can see that 1 mole of N2O4 decomposes to produce 2 moles of NO2.
If we start with 2.35 moles of N2O4, we can use the mole ratio from the equation to find out how many moles of NO2 are produced:
\[
\text{Moles of NO2} = 2.35 \, \text{moles of N2O4} \times \frac{2 \, \text{moles of NO2}}{1 \, \text{mole of N2O4}} = 4.70 \, \text{moles of NO2}
\]
Therefore, when 2.35 moles of N2O4 are decomposed, **4.70 moles of NO2 are produced**.
\[
N2O4 \rightarrow 2NO2
\]
From the balanced equation, we can see that 1 mole of N2O4 decomposes to produce 2 moles of NO2.
If we start with 2.35 moles of N2O4, we can use the mole ratio from the equation to find out how many moles of NO2 are produced:
\[
\text{Moles of NO2} = 2.35 \, \text{moles of N2O4} \times \frac{2 \, \text{moles of NO2}}{1 \, \text{mole of N2O4}} = 4.70 \, \text{moles of NO2}
\]
Therefore, when 2.35 moles of N2O4 are decomposed, **4.70 moles of NO2 are produced**.