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The balanced equation for the reaction of nitrogen dioxide and fluorine is given below: 2 NO2...

The balanced equation for the reaction of nitrogen dioxide and fluorine is given below: 2 NO2 + F2 → 2 NO2F The proposed mechanism is: step 1: NO2 + F2 → NO2F + F (slow) step 2: F + NO2 → NO2F (fast) Based on this information, the following observations are made: I. The mechanism supports an experimentally determined rate law of rate = k[NO2]2[F2] II. F is an intermediate III. The reaction is first order in F2 Which of these observations is accurate?

Given the following equilibrium constants,

Zn(IO3)2 Ksp = 3.9 x 10¯6

Zn(NH3)42+ Kf = 2.9 x109

determine Kc for the dissolution of the sparingly soluble salt Zn(IO3)2 in aqueous ammonia (shown below).

Zn(IO3)2 (s) + 4NH3 (aq) ↔ Zn(NH3)42+ (aq) + 2IO3– (aq)

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