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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?

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Answer 1 · 2018-06-26T04:22:56

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

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 $R_("inst") = 4.64*10^(-6) M^(-2)s^(-1)$