# I need some help?

## The following reaction is first order in H2 and second order in NO with a rate constant of $2.9 \cdot {10}^{2} {M}^{- 2} \cdot {s}^{- 1}$. $2 N {O}_{g} + {H}_{2 \left(g\right)} \rightarrow {N}_{2} {O}_{\left(g\right)} + {H}_{2} {O}_{\left(g\right)}$ Calculate the instantaneous rate when the reactant concentration $\left[N O\right] = 0.00200 M$ and $\left[{H}_{2}\right] = 0.00400 M$. What is the overall order of the reaction?

Jun 26, 2018

Order of reaction is 3 and instantaneous rate(${R}_{\text{inst}}$)$= 4.64 \cdot {10}^{- 6} {M}^{- 2} {s}^{- 1}$

#### Explanation:

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

$\text{Rate of reaction} = K \left[{H}_{2}\right] {\left[N O\right]}^{2}$

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

Substituting $\left[N O\right] = 0.00200 M , \left[{H}_{2}\right] = 0.00400 M , K = 2.9 \cdot {10}^{2} {M}^{- 2} {s}^{- 1}$,we get ${R}_{\text{inst}} = 4.64 \cdot {10}^{- 6} {M}^{- 2} {s}^{- 1}$