Asked by Steve
Nitrogen dioxide reacts with carbon monoxide to produce nitrogen monoxide and carbon dioxide.
NO2(g) + CO(g) ==>NO(g) + CO2(g)
A proposed mechanism for this reaction is
2No2(g) = NO3(g) + NO(g) (fast,equilibrium)
NO2(g) + CO(g) ==> NO2(g) + CO2(g) (slow)
The rate law consitent with the propose mechanism is
rate = k[NO2]^2[CO]/[NO]
How?
NO2(g) + CO(g) ==>NO(g) + CO2(g)
A proposed mechanism for this reaction is
2No2(g) = NO3(g) + NO(g) (fast,equilibrium)
NO2(g) + CO(g) ==> NO2(g) + CO2(g) (slow)
The rate law consitent with the propose mechanism is
rate = k[NO2]^2[CO]/[NO]
How?
Answers
Answered by
DrBob222
1.The two equations you have written does not add to the final equation. Something is amiss.
2. I haven't seen any rate equations that look like equilibrium constants.
Check your post please.
2. I haven't seen any rate equations that look like equilibrium constants.
Check your post please.
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