For the reaction of nitric oxide, NO with chlorine, $Cl_2$ : $2NO(g)$ + $Cl_2(g)$ $rarr$ $2NOCl(g)$ The observed rate law is R = k $[NO]^2$ $[Cl_2]$ a) What is the reaction order with respect to nitric oxide? with respect to chlorine? and the overall order?

Question

b) What will happen to the rate if the concentration of the nitric oxide is doubled?
c) What will happen to the rate of the concentration of both nitric oxide and chlorine are doubled?
Thank you so much in advance. :)

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Answer 1 · 2018-02-25T06:22:23

order of reaction w.r.t $NO$ is indicated by the power depicted in the rate equation,it is $2$

Similarly from the equation, $R=k[NO]^2 [Cl_2]$ we can say the power of $Cl_2$ is $1$ ,so order of rxn,w,r,t it is $1$

Overall order is the sum of the power i.e $2+1=3$

Now,let,the rate ( $R'$ ) after doubling the conc of $NO$ would be,

$R'= k[2NO]^2 [Cl]=4*k[NO]^2 [Cl]=4R$

And,the rate constant will be $R''$ when conc of both are doubled,

so, $R''=k[2 NO]^2 [2 Cl] = 8 k[NO]^2 [Cl]=8R$

So,now we can say,if the conc of $NO$ is doubled,its rate will be $4$ times the previous, and when both of them are doubled it will be $8$ times