Answer :
Answer
2.24 L
Explanation
Given:
volume of nitrogen dioxide produced = 4.50 L
The given unbalanced equation is;
___ NO (g) + ___O2 (g) → ___NO2 (g)
What to find:
The liters of gaseous oxygen needed to produce 4.50 L of gaseous nitrogen dioxide at STP.
Step-by-step solution:
The first step is to write a balanced equation for the reaction.
2 NO (g) + 1 O2 (g) → 2 NO2 (g)
The next step is to convert 4.5 L NO2 to moles.
Conversion factor: 1 mole of any gas at STP occupies 22.4L.
Therefore, the number of moles of NO2 in 4.5 L volume will be
[tex]\frac{4.5L}{22.4L}\times1mol=0.20\text{ }mol\text{ }NO_2[/tex]The next step is to calculate the mole of O2 needed to produce 0.20 mol NO2.
From the balanced equation 1 mol O2 produce 2 mol NO2
So, the x mol O2 will be needed to prduce 0.20 mol NO2
[tex]\frac{0.20mol\text{ }NO_2}{2mol\text{ }NO_2}\times1mol\text{ }O_2=0.1mol\text{ }O_2[/tex]The final step is to convert 0.1 mol O2 to liters using the conversion factor in step 2.
The liters of gaseous oxygen needed is
[tex]\frac{0.1mol}{1mol}\times22.4L=2.24\text{ }L[/tex]The liters of gaseous oxygen needed to produce 4.50 L of gaseous nitrogen dioxide at STP = 2.24 L
