What is the rate law for the following mechanism in terms of the overall rate constant kk?
Step1:Step2:A+BB+C⇌→CD(fast)(slow)Step1:A+B⇌C(fast)Step2:B+C→D(slow) |
What is the rate law for the following mechanism in terms of the overall rate constant...
A reaction mechanism is defined as the sequence of reaction steps that define the pathway from reactants to products. Each step in a mechanism is an elementary reaction, which describes a single molecular event of usually one or two molecules interacting. The rate law for an overall reaction is the rate law for the slowest step in the mechanism, which is directly related to the stoichiometric coefficients of the reactants. The exception to this rule occurs when the slowest step...
Consider the following mechanism. step 1 2A > B slow B+ C D fast step 2 overall: 2A+C D Determine the rate law for the overall reaction (where the overall rate constant is represented as k) rate=
What is the rate law for overall reaction? Consider the following mechanism: Step 1: 03 → 02 + 0 Step 2: 03 + 0 + 2O2 (fast) (slow)
Part A Given the following proposed mechanism, predict the rate law for the overall reaction. 2 NO2 + Cl2 → 2 NO2Cl (overall reaction) Mechanism NO2 + Cl2 → NO2Cl + Cl slow NO2 + Cl → NO2Cl fast Given the following proposed mechanism, predict the rate law for the overall reaction. 2 NO2 + Cl2 → 2 NO2Cl (overall reaction) Mechanism NO2 + Cl2 → NO2Cl + Cl slow NO2 + Cl → NO2Cl fast Answer Choices: Rate =...
Consider the overall reaction.... A+B--C+D which has an observed rate law of Rate=k[A12 Which of the following choices would be a sensible 2-step mechanism, given this observed rate law? O A+A-->E slow E+B-->C+D fast A+B--> 2 E --> C+D fast slow A+A-->E E+B-->C+D fast slow A+B-->E 2 E -->C+D slow fast
Consider the following mechanism. Step 1: A+B → C slow step 2: A+C→ D fast overall: 2A+B → D Determine the rate law for the overall reaction (where the overall rate constant is represented as k). rate w
Consider the mechanism. 2A - B slow Step 1: Step 2: Overall: B + C -→ D fast 2 A + C -- D Determine the rate law for the overall reaction, where the overall rate constant is represented as k.
For the overall reaction below, which of the following is the correctly written rate law? Overall reaction: O3(g)+2NO2(g)→N2O5(g)+O2(g) Step 1: O3(g)+NO2(g)→NO3(g)+O2(g) slow Step 2: NO3(g)+NO2(g)→N2O5(g) fast View Available Hint(s) For the overall reaction below, which of the following is the correctly written rate law? Overall reaction: Step 1: slow Step 2: fast A.] Rate=k[O3][NO2]2 B.] Rate=k[O3][NO2] C.] Rate=k[NO3][NO2] D.] Rate=k[O3][NO2]2[N2O5][O2]
Consider the mechanism. Step 1: AB+C Step 2: C+ DE Overall: A+D- B+E slow fast Determine the rate law for the overall reaction, where the overall rate constant is represented ask. rate =
In a hydrocarbon solution, the gold compound (CH3)3AuPH3 decomposes into ethane (C2H6) and a different gold compound, (CH3)AuPH3. The following mechanism is proposedfor the decomposition of (CH3)3AuPH3.Step 1:(CH3)3AuPH <-----> (CH3)3Au + PH3 (fast)Step 2:(CH3)3Au -----> C2H6 + (CH3)Au (slow)Step 3:(CH3)Au + PH3 ------>(CH3)AuPH3 (fast)A)What is the overall reaction?B)What are the intermediates in the mechanism?C)What is the rate law predicted by this mechanism?Use a for :(CH3)3AuPH , b for (CH3)3Au, c for PH3, d for C2H6 , e for (CH3)Au and...