Nitirc oxide, NO, reacts with oxyegen to producenitrogen dioxide. 2NO (g) + O 2(
ID: 682653 • Letter: N
Question
Nitirc oxide, NO, reacts with oxyegen to producenitrogen dioxide. 2NO(g)+ O2(g) ----> 2NO2(g) (overallequation) If the mechanism is k1 NO + O2 <----> NO3 (fast,equilibrium) k-1 k2 NO3+ NO ----> NO2 + NO2 (slow) What is theperdicted rate law? Remember to express this in terms ofsubstances in the chemical equilibrium equation! Nitirc oxide, NO, reacts with oxyegen to producenitrogen dioxide. 2NO(g)+ O2(g) ----> 2NO2(g) (overallequation) If the mechanism is k1 NO + O2 <----> NO3 (fast,equilibrium) k-1 k2 NO3+ NO ----> NO2 + NO2 (slow) What is theperdicted rate law? Remember to express this in terms ofsubstances in the chemical equilibrium equation! k2 NO3+ NO ----> NO2 + NO2 (slow) What is theperdicted rate law? Remember to express this in terms ofsubstances in the chemical equilibrium equation!Explanation / Answer
Rate determining step is the slowest step rate = k[NO3][NO] Noticed that NO is in the equilibrium reaction (the firstequation), but NO3 is not For the fast reaction: Rate = k[NO][O2] Rate = k-1[NO3] Since they are at equilibrium, the rate are equal, so set the twoequations equal to one another k[NO][O2]=k-1[NO3] [NO3]=(k)[NO][O2], where k/k-1 can also be written as "k" for a newconstant rate Plug back into the original one above rate = k(k[NO][O2])[NO], k2 can also just be written as"k" as the new constant. Final: rate =k[NO]2[O2] To check: noticed that both NO and O2 are in the equilibriumequation.
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