Suppose the decomposition of dinitrogen monoxide proceeds by the following mechanism:
step. elementary reaction. rate constant
1. n2o(g)=n2(g)+o(g). k1
2. n2o(g)+o(g)=n2(g)+o2(g). k2
suppose also k1<
write the balance chemical question for the overall chemical reaction:

write the experimental observable rate law for the overall chemical reaction. know your answer should not contain the concentrations of any intermediates.

express the rate constant k for the overall chemical reaction in terms of k1, k2 and if necessary the reconnaissance k -1 and k -2 for the reverse of the two elementary reactions in the mechanism.

Many reactions take place in aqueous solution. when potential reactants are mixed, a reaction will occur if there is some driving force that favors the formation of products. it is often convenient to categorize reactions in terms of these driving forces: precipitate formation, in which an insoluble solid is formed, weak electrolyte formation, as in a neutralization reaction involving water, or transfer of electrons, as in a redox reaction. these reactions can be represented by full molecular equations, which contain all species in the reaction mixture, or by net ionic equations, which show only the species that actually undergo a change. the latter does not contain the spectator ions, which do not undergo a net change or do not take part in the reaction. part a when the following two solutions are mixed: k2co3(aq)+fe(no3)3(aq) the mixture contains the ions listed below. sort these species into spectator ions and ions that react. drag the appropriate items to their respective bins. view available hint(s) spectator ions ions that react part b what is the correct net ionic equation, including all coefficients, charges, and phases, for the following set of reactants? assume that the contribution of protons from h2so4 is near 100 %.ba(oh)2(aq)+h2so4(aq)→ express your answer as a chemical equation. view available hint(s) nothing provide feedback