Answer:
[tex]r_{N_2O_5}=-4.00mol/min\[/tex]
Explanation:
Hello.
In this case, since the chemical reaction is:
[tex]2N_2O_5\rightarrow 4NO_2+O_2[/tex]
We can write the rate ratio between N2O5 and NO2 as shown below:
[tex]\frac{1}{-2} r_{N_2O_5}= \frac{1}{4} r_{NO_2}[/tex]
Since N2O5 is consumed and NO2 produced at a rate of 8.00 mol/s, therefore, the rate of disappearance is N2O5 is:
[tex]r_{N_2O_5}= \frac{-2}{4} r_{NO_2}\\\\ r_{N_2O_5}=\frac{-1}{2} *8.00 mol/min\\\\ r_{N_2O_5}=-4.00mol/min[/tex]
Which is negative since N2O5 is a reactant.
Best regards!
