Question

I need some help?

The following reaction is first order in H2 and second order in NO with a rate constant of `2.9 * 10^2 M^(-2)*s^(-1)`.
`2NO_(g) + H_(2(g)) rarr N_2O_((g)) + H_2O_((g))`
Calculate the instantaneous rate when the reactant concentration `[NO]=0.00200M` and `[H_2]=0.00400M`. What is the overall order of the reaction?

Answer 1

Order of reaction is 3 and instantaneous rate(`R_("inst")`)`=4.64*10^(-6) M^(-2)s^(-1)`

Explanation:

According to question,order with respect to hydrogen is 1 and order with respect to NO is 2.So, according to Rate law,

`"Rate of reaction"=K[H_2][NO]^2`

From above rate equation, it is clear that order of reaction is 3 .

Substituting `[NO]=0.00200M, [H_2]=0.00400M, K=2.9*10^2 M^(-2)s^(-1)`,we get `R_("inst") = 4.64*10^(-6) M^(-2)s^(-1)`