Consider the following fictitious mechanism: Step 1. R+S T, (fast, reversible) Step 2. T +U -...
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
#13 Interpreting Mechanisms 1. Consider the following mechanism: Step 1 Br2 2Br fast Step 2 Br + H2 H2Br fast Step 3 H2Br + Br 2HBr slow a. What is the overall equation? b. Identify the intermediate(s) if any. c. What is the molecularity and the rate law for each step including any reversible steps? d. What is the predicted rate law expression for this reaction. Be sure to only list reactants from the overall equation and...
2. Consider this two step mechanism for a reaction… Step 1 NO2 + O3 --> NO3 + O2 slow; rate determining step Step 2 NO3 + NO2 --> N2O5 fast a. What is the overall reaction? b. Identify the intermediates in the mechanism. c. Write the rate law expression for each step of the mechanism including any reversible reactions. c. What is the predicted rate law expression? Be sure to only list reactants from the overall equation and not intermediates...
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=
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 =
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 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.
A proposed mechanism for a reaction is as follows: NO2(g) + NO2(g) + N204(8) Fast/Equilibrium Step N2048) -> NO(g) + NO3(g) Slow NO3(g) NO) + O2(g) Fast The target rate law is rate = k (NO2)2 The target reaction is 2NO2(e) 2NON + O2) A. Write the rate law expected for this mechanism: B. What is the rate-determining step? C. What is the overall balanced equation for this mechanism? D. If there is/are a reactive intermediate(s), which is/are they? E....
Consider the following three step mechanism for a reaction Cl2 > 2Cl Fast Cl+CHCl3 > HCl+CCl3 Slow Cl+CCl3 > CCl4 Fast What is the predicted rate law? How do you do it? The answer is rate=K[Cl2]^.5 [CHCl3]
Suppose a reaction occurs with the following mechanism: Step 1: 2AD Step 2: D+E- (fast) B+C (slow) 1. What is the overall reaction? [Select] 2. What is the intermediate in the mechanism? (Select] 3. What is the molecularity of step 1? (Select 4. Which step is the rate determining step? [Select) 5. What is the rate law predicted by this mechanism? [Select) Question 22 15 pts Consider the following reaction at equilibrium: CO(g) + 2H2(g) CH2OH(g) AH=-18 kJ How will...