# The experimental rate law for the reaction 2H2(g) + 2 NO(g) → N2(g) +2 H2O(g) is...

###### Question:

The experimental rate law for the reaction 2H2(g) + 2 NO(g) → N2(g) +2 H2O(g) is d[N2) = kods[Hz][NO] Below is a proposed mechanism: H2(g) + NO(g) + NO(g) = N2O(g) + H2O(g) H2(g) + N2O(g) = N2(g) + H2O(g) ki k2 (a) Under what conditions does this mechanism give the observed rate law? Express kobs in terms of the rate constants for the individual steps of the mechanism. A second proposed mechanism is: NO(g) + NO(g) = N2O2(g) N2O2(g) = NO(g) + NO(g) H2(g) + N2O2(g) = N2O(g) + H2O(8) H2(g) + N2O(g) = N2(g) + H2O(g) (b) Under what conditions does this mechanism give the observed rate law? Express kobs in terms of the rate constants for the individual steps of the mechanism. Do you favour this mechanism or the first one? Explain your reasoning.

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