Write the rate law for the following elementary reaction:

2n2o5(g) - 2n204 use k1 to stand for the rate constant.

Rate law = k1 [N2O5]^2

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

i just got this problem. it's 90.3

oxygen, selenium, tellurium, and polonium.

they're all from the same group as sulfur (group 16).