Question

The instantaneous rate data in Table 3 were obtained for

the reaction H2(g) + 2NO(g) →H2O(g) + N2O(g) at a
given temperature and concentration of NO. How does
the instantaneous rate of this reaction change as the
initial concentration of Hy is changed? Based on the
data, is [Hz] part of the rate law? Explain.

Answer 1

A) As the initial concentration of H₂ is increased, the reaction rate also increases.

B) Yes, [H₂] is part of the rate law.

Step-by-step explanation:

For the reaction:

`\displaystyle \text{H$_2$}_\text{(g)} + 2\text{NO}_\text{(g)} \longrightarrow \text{H$_2$O}_\tex{(g)} + \text{N$_2$O}_\text{(g)}`

The rate law will have the form:

`\displaystyle \text{Rate} = k\left[\text{H$_2$}\right]^n\left[\text{NO}\right]^m`

Where n and m are the respective order of reactions.

From the table, we can see that as the concentration of H₂ increases, the instantaneous rate also increases.

Therefore, [H₂] is indeed part of the rate law. If it isn't, changing its concentration will have no effect on the instantaneous rate of the reaction.