Nitrogen monoxide reacts with oxygen gas to form nitrogen dioxide. 2 NO(g) + O2(g)2 NO2(g) Determine the rate law for the following mechanism. Step 1, Fast equilibrium NO(g) + O2(g) → OONO(g) Step 2, Slow NO(g) + OON0(g)→ 2 NO2(g) Rate

Q: What are the units of k in the following rate law? Rate = k[X][Y] %3D M3 Ms 一。

A: To solve this problem we will use the given rate law   Rate = k[X][Y] .

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Q: Nitrogen(II) oxide reacts with chlorine according to the equation: 2NO(g) + Cl2(g) – 2NOCI(g) The…

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Q: Nitrogen monoxide, NO, reacts with hydrogen, H, according to the following equation: 2NO+2H→N+ 2H,O…

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Q: Step 1 X + Y XY (slow) Step 2 XY + Y → XY2 (fast)

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Q: [References] Nitryl chloride, NO2CI, decomposes into nitrogen dioxide and chloride. 2NO, Cl(g) →…

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Q: 1. Nitrosyl chloride, NOCI, decomposes to NO and Cl2. 2NOCI(g) → 2NO(g) + Cl, (g) Determine the rate…

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Q: Consider the mechanism. O, + NO, → NO, + O, slow NO, + NO, → N,O5 fast O, + 2 NO, → O, + N,O5 -…

A: The mechanism given is,

Q: What are the units of k in the following rate law? Rate = k[X] [Y]

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A: For a given Chemical Reaction , Rate law is given by  Rate = [A]q [B]r [C]s