4. The dissociation of NO2 occurs by the following reaction: 2NO2(g) → 2NO(g) + O2(g) If the rate for the reaction is 0.83 M sl, i. Write the differential rate expression for the above reaction. ii. Determine the rate of disappearance of NO2. [4M]

a. This can be gotten from the equation of reaction. An easy way about this is always consider the reactant dissipating and carries a negative sign while the foward reaction carries the postive sign since products is formed.

The differential rate of the reaction can be written as

[tex]-\frac{1}{2}\frac{d}{dt}\lbrack NO_2\rbrack=-\frac{1}{2}\lbrack NO\rbrack=\frac{d}{dt}\lbrack O_2\rbrack[/tex]

b.

But the rate ofthe reaction is

[tex]\begin{gathered} r=k\lbrack NO_2\rbrack^2 \\ r=0.83Ms^{-1} \end{gathered}[/tex]

Now, let's bring the differential equation back

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