The nitrogen-monoxide-catalyzed decomposition of dinitrogen
monoxide is thought to proceed by a two-step mechanism:
NO(g) + N2O(g) --> N2(g) +
NO2(g) (slow)
2 NO2(g) --> 2 NO(g) + O2(g)
(a) If the first step of this mechanism is rate-determining (slow),
choose the correct rate law for the overall process.
Rate = k [N2O]2
Rate = k [NO] [NO2]
Rate = k [N2O]2 [N2O]
Rate = k [NO2] [N2O]
Rate = k [N2O] [N2O]
Rate = k [NO] [N2O]
(b) Choose the correct chemical equation for the overall
process.
2 NO2(g) --> 2 NO(g) + O2(g)
NO(g) + N2O(g) --> N2(g) + NO2(g)
2 N2O(g) --> 2 N2(g) + O2(g)
(c) Identify an intermediate in the reaction.
N2
NO2
NO
N2O
(d) Identify the catalyst in the reaction.
N2O
NO2
N2
NO
(e) Identify a reactant in the reaction.
NO2
N2O
NO
N2
(f) Identify a product in the reaction.
N2O
NO
NO2
N2
The nitrogen-monoxide-catalyzed decomposition of dinitrogen monoxide is thought to proceed by a two-step mechanism: NO(g) +...
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Can check my answrs as well if it's correct and help me out with the last part of the question. Suppose the decomposition of dinitrogen monoxide proceeds by the following mechanism: step elementary reaction rate constant ki N2O(g) → N2(9) + O(g) 2 N2O(g) + 0(g) N2(g) + O2(9) k Suppose also k,«k2. That is, the first step is much slower than the second. Write the balanced chemical equation for the overall chemical reaction: 2N 0(3) 2N, (g) + 02...
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