2Cl(g) fast Cl(g) + CHCl3(g) > HCl(g) + CCl3(g) slow Cl(g) + CCl3(g) > CCl4(g) fast  A) Use the above equation to determine the overall reaction. B) Identify the intermediates in the mechanism.

A) In the proposed reaction mechanism below, the intermediate product is: A).  NO(g) B).  N2O2(g) C).  H2(g) D).  N2O(g)   B) The rate expression for a particular reaction is rate = k[A][B]^2. If the initial concentration of B is increased from 0.10M to 0.30M, the initial rate will increase by which of the following factors  A) 2 B) 3 C) 6 D) 9

H2 reacts with ClF. Someone thinks this is the mechanism:                               H2(g)  +  ClF(g) → HCl(g)  + HF(g)                               HCl(g)  +  ClF(g) →  Cl2(g)   + HF(g) (a)     Write the balanced equation for the overall reaction. (b)  Identify any intermediates in the mechanism, if any. (c) identify and catalysts in the mechanism, if any. (d) Write rate laws for each elementary reaction in the mechanism. (e)  If the first step is slow and the second one is fast, what rate law do you expect to be observed for the overall reaction?

What is the rate law of the reaction                         NO2(g)    +    CO(g)   ó   NO(g)   +   CO2(g)       If the mechanism behind it is : 2NO2(g) à   2NO(g)   +   O2(g)          (slow) NO(g) +   CO(g)   +   O2(g)   à   NO2(g)   +   CO2(g)       (fast)   Rate of reaction is rate of slow step.   Rate = k [NO2]2

The following mechanism has been proposed for the atmospheric destruction of ozone, O3 (g):O3 (g) + NO (g) --> O2 (g) + NO2 (g) (slow)NO2 (g) + O (g) --> NO (g) + O2 (g) (fast)a) Write the equation for the overall balanced reaction. b) Write the rate law predicted by this reaction mechanism.

The following mechanism has been proposed for the reaction of H2 (g) and NO (g): H2 (g) + NO (g) → H2O (g) + N (g) (Slow)N (g) + NO (g) → N2 (g) + O (g) (Fast)H2 (g) + O (g) → H2O (g) (Fast)a) Write the equation for the overall balanced reaction. b) Write the rate law predicted by this reaction mechanism.

The following is a proposed reaction mechanism for the decomposition of BrO2: 1          BrO2 + CO --> CO2 + BrO                                                 2          2BrO2 --> BrO + BrO3 3          BrO3 + CO --> CO2 + BrO2 a) If the rate law for this reaction is: Rate = k[BrO2], what is the rate determining step?  How do you know? b) What is the overall reaction based on this mechanism? c) What are the intermediates, if any?             d) What are the catalysts, if any?

Consider the reaction: 2NO(g) + O2(g) → 2NO2(g) Suppose that a particular moment during the reaction nitric oxide (NO) is reacting at a rate of 0.022 M/s. At what rate is molecular oxygen reacting? M Molecular oxygen is (select) at a rate of