The decomposition of nitramide, O2NNH2, in water has the following chemical equation and rate law.

Print Calculator Periodic Table O,NNH, Map A proposed mechanism for this reaction is (fast equilibrium) (1) ONNHz(aq) ê·¼ã2NNH-(aq)+H+(aq) (2) o,NNH-(aq)âN,ole) +OH,(aq) (3) H.(aq)+OH-(aq) â H2O(1) (slow) (rast) Determine the rate law for each elementary s Drag the symbols into the equations as Which of these rates is equal to the overall reaction rate? rate, = O rater O rate2 rates [H'T rate,- [H-O] O Previous Give Up & View Solution 9 Check Answer Next -H Exa Hint

answer

watching

638

views

For unlimited access to Homework Help, a Homework+ subscription is required.

You have 0 free answers left.
Get unlimited access to 3.8 million step-by-step answers.

Get unlimited access

Already have an account? Log in

Tod ThielLv2

10 Oct 2019

Unlock all answers

Get 1 free homework help answer.

Already have an account? Log in

Join us on Discord

Chemistry Study Group

Join now

Related questions

coffeepug497

The decomposition of nitramide, O2NNH2, in water has the following chemical equation and rate law. O2NNH2 (aq) yields N2O (g) + H2O (l) rate= [O2NNH2]/[H]A proposed mechanism for this reaction is.k1(1) O2NNH2 (aq) equilibrium O2NNH (aq) + H (aq) (fast equilibrium)k-1k2(2) O2NNH (aq) yields N2O (g) + OH (aq) (slow)k3(3) H (aq) + OH yields H2O (l) (fast)What is the relationship between the observed value of k and the rate constants for the individualsteps of the mechanism?k=__________Also which symbols go into the numerator or demoniator k-1, k3, k2, k1