Question

Write the rate law for the following elementary reaction:

2N2O5(g) - 2N204 Use k1 to stand for the rate constant.

Answer 1

The rate law for the reaction 2N2O5(g) → 2N2O4(g) is rate = k1[N2O5]^2, indicating a second-order dependence on [N2O5]. For the reaction H2(g) + 2NO(g) → N2O(g) + H2O(g), the rate law is rate = k[NO]^2[H2], with the reaction being second order in NO and first order in H2.

Step-by-step explanation:

The rate law for an elementary reaction can be written directly from the stoichiometry of the reaction. Considering the provided elementary reaction 2N2O5(g) → 2N2O4(g), the rate law would be rate = k1[N2O5]^2, which indicates that the reaction is second order with respect to N2O5.

In general, for an elementary reaction like H2(g) + 2NO(g) → N2O(g) + H2O(g), the rate law given is rate = k[NO]^2[H2], which means that the reaction is second order with respect to NO (order of 2) and first order with respect to H2 (order of 1), making the overall order of the reaction three.

Answer 2

Rate law = k1 [N2O5]^2

Step-by-step explanation:

Rate law only cares about reactants and rate law can only be determined experimentally or by using the coefficients of reactants in elementary reactions

If 2A---->B is an elementary reaction... rate law for this is rate=k[A]^2

So if we look at your question...2N2O5---->2N2O4 + 02 (I think you are missing O2 in question because otherwise equation is unbalanced)

Rate law = k1 [N2O5]^2