The reaction, 2 NO(g) + Cl2(g) --> 2 NOCl(g), proceeds through the following mechanism:   NO(g) + Cl2(g) --> NOCl2(g) NOCl2(g) + NO(g) --> 2 NOCl(g) The second step of this mechanism is rate-determining (slow). What would the rate law for this reaction be if the first step were rate-determining

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

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