For the proposed reaction mechanism shown below what is the overall chemical equation predicted by this mechanism and what is the rate law derived from this mechanism? Hint: The slow step determines the overall rate then see if there is a possible substitution for one of the reactant. When you get to the equilibrium reaction write the rate law in terms of [N2O5] and then substitute this back into the overall rate equation. (slow step, K1 N205 → NO2 + NO3 forward rate) (fast step, K2 forward rate) NO2 + NO3 → NO2 + O2 + NO (fast step, equilibrium, K3 forward rate, K3 = NO + N205 → 3NO2

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For the proposed reaction mechanism shown below what is the overall chemical equation predicted
by this mechanism and what is the rate law derived from this mechanism? Hint: The slow step
determines the overall rate then see if there is a possible substitution for one of the reactant.
When you get to the equilibrium reaction write the rate law in terms of [N205] and then substitute
this back into the overall rate equation.
(slow step,
K1
N205 → NO2 + NO3
forward
rate)
(fast step,
K2
NO2 + NO3 → NO2 + O2 + NO
forward
rate)
(fast step,
equilibrium,
K3
NO + N205
3NO2
forward
rate, K_3
reverse
Transcribed Image Text:For the proposed reaction mechanism shown below what is the overall chemical equation predicted by this mechanism and what is the rate law derived from this mechanism? Hint: The slow step determines the overall rate then see if there is a possible substitution for one of the reactant. When you get to the equilibrium reaction write the rate law in terms of [N205] and then substitute this back into the overall rate equation. (slow step, K1 N205 → NO2 + NO3 forward rate) (fast step, K2 NO2 + NO3 → NO2 + O2 + NO forward rate) (fast step, equilibrium, K3 NO + N205 3NO2 forward rate, K_3 reverse
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