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(a) From the differential rate equation given below, write a balanced equation for the reaction involved. 1 d[N o,) i d[NO] d[0] N2011 2 2 dt 4 dt dt rate (b) Given, rate = k[NO2]2[Cl2], by what factor does the rate increase of each of the following changes occurs. i. (NO2) is tripled. ii. [NO2] and [Cl2] are doubled [4M]

A From The Differential Rate Equation Given Below Write A Balanced Equation For The Reaction Involved 1 DN O I DNO D0 N2011 2 2 Dt 4 Dt Dt Rate B Given Rate KNO class=

Sagot :

We are given an equation that shows the differential rate change of the reaction and it is given as

[tex]-\frac{1}{2}\frac{d}{dt}\lbrack N_2O_5\rbrack=\frac{1}{4}\frac{d}{dt}\lbrack NO_2\rbrack=\frac{d}{dt}\lbrack O_2\rbrack[/tex]

This depicts the decomposition reaction of Nâ‚‚Oâ‚…. The forward reaction (product) carries a positive sign while the backward reaction or (reactant) carries a negative sign.

We can as well integrate this, but for the sake of simplicity, the equation of reaction is given as

[tex]2N_2O_5\rightleftarrows4NO_2+O_2[/tex]

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