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Reaction 1 below occurs very slowly, while reaction 2 below occurs much more rapidly: 1. O2(g) → 20 (9) 2. Ar(g) + O2(g) → ArPlease make sure these both are correct I keep getting different answers, make sure it is not wrong the answer you give. THANKSConsider the following reaction mechanism: Step 1 K 2A + B =D (fast equilibrium) Step 2 D+B *? E + F (slow) Step 3 F G (fast)c. What is the rate law that corresponds to this mechanism assuming the first step is at equilibrium? O rate = k2K1[A] [B]? Od. Here are some initial velocity data for this reaction. Experiment [A]. (M) [B]. (M) rate (M.3-1) 1 0.50 0.50 10. 2 0.25 0.

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