# Question #3d50a

Dec 5, 2017

Chemical reaction:$2 N {O}_{g} + {O}_{2} \Rightarrow 2 N {O}_{2} \left(g\right)$
As we can see: for the reaction of 1 mole oxygen requires 2 moles of NO
The initial concentration of NO$\rightarrow$0.03$\frac{m o l}{{\mathrm{dm}}^{3}}$
and ${O}_{2} \Rightarrow 0.04 \frac{m o l}{{\mathrm{dm}}^{3}}$
In this reaction NO is limiting reactant because 0.04$\frac{m o l}{{\mathrm{dm}}^{3}}$ oxygen reacts with 0.08$\frac{m o l}{{\mathrm{dm}}^{3}}$ of NO
But The initial concentration of NO$\rightarrow$0.03$\frac{m o l}{{\mathrm{dm}}^{3}}$
The concentration of products formed depends on that of NO

when 0.01$\frac{m o l}{{\mathrm{dm}}^{3}}$ reacted the concentration of NO reacted is 0.02$\frac{m o l}{{\mathrm{dm}}^{3}}${according to stotiometry}to give 0.02$\frac{m o l}{{\mathrm{dm}}^{3}}$ product NO2

$N {O}_{2} f \mathmr{and} m e d \rightarrow 0.02 \frac{m o l}{{\mathrm{dm}}^{3}}$
NO left$\rightarrow$0.01$\frac{m o l}{{\mathrm{dm}}^{3}}$
O2 left$\rightarrow$0.03-0.01=0.02$\frac{m o l}{{\mathrm{dm}}^{3}}$