Nitrogen monoxide reacts with ozone: NO(g) + O3g) right arrow NO2(g) + O2(g) Two

Question

Nitrogen monoxide reacts with ozone: NO(g) + O3g) right arrow NO2(g) + O2(g) Two mechanisms have been proposed: Mechanism I (one step): NO(g) + O3(g) right arrow NO2(g) + O2(g) Rate law: reaction rate = k[NO]^x [O3]^Y What are x and y? Nitrogen monoxide reacts with ozone: NO(g) + O3g) right arrow NO2(g) + O2(g) Two mechanisms have been proposed: Mechanism I (one step): NO(g) + O3(g) right arrow NO2(g) + O2(g) Rate law: reaction rate = k[NO]^x [O3]^Y What are x and y? Mechanism II(two steps): O3(g) right arrow O2(g) + O(g) slow NO(g) + O(g) right arrow NO2(g) Rate law: reaction rate = k[NO]^X [O3]^Y What are x and y?

Explanation / Answer

rate depends on slowest step.
rate= k [O3]

so, x=0 and y=1

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