Consider the following three-step mechanism for a reaction: Br2 (g) ⇌ 2 Br (g) Fast Br...

Consider the following three-step mechanism for a reaction:
Br₂ (g) ⇌ 2 Br (g) Fast
Br (g) + CHBr₃ (g) → HBr (g) + CBr₃ (g) Slow
Br (g) + CBr₃ (g) → CBr₄ (g) Fast

Based on this mechanism, determine the rate law for the overall reaction.

Rate =

Solutions

Expert Solution

Using the three step mechanism for the given reaction

, the slowest step is the rate determing step for the reaction shown

whereas the fast step are not the rate determining step, so the rate law for the given mechanism can be stated as

Rate = [CHBr3][Br]

queen_honey_blossom answered 1 year ago

Next > < Previous

Related Solutions

The rate determining step in a reaction mechanism: A. is the fast step B. is the...

The rate determining step in a reaction mechanism: A. is the fast step B. is the slow step C. is always the first step D. is the transition state

Consider the following two-step mechanism for a reaction: NO2(g)+Cl2(g)→ClNO2(g)+Cl(g)Slow NO2(g)+Cl(g)→ClNO2(g)Fast 1)What is the overall reaction? Express...

Consider the following two-step mechanism for a reaction: NO2(g)+Cl2(g)→ClNO2(g)+Cl(g)Slow NO2(g)+Cl(g)→ClNO2(g)Fast 1)What is the overall reaction? Express your answer as a chemical equation. Identify all of the phases in your answer. 2)Identify the intermediates in the mechanism. 3)What is the predicted rate law?

Consider this two step mechanism for a reaction

Consider this two step mechanism for a reaction Step 1 NO2 + Cl2 ---------> ClNO2 + Cl slow; rate determining step Step 2 NO2 + Cl ---------> ClNO2 fast a. What is the overall reaction? b. Identify the intermediates in the mechanism. c. What is the predicted rate law expression? Be sure to only list reactants from the overall equation and not intermediates in the rate law expression.

A proposed mechanism for the preparation of COBr2 from CO(g) and Br2 is: Br2 ⇄ 2...

A proposed mechanism for the preparation of COBr2 from CO(g) and Br2 is: Br2 ⇄ 2 Br (g) fast Br(g) + CO (g) ⇄ COBr fast COBr + Br2 → COBr2 + Br slow The correct rate law for this mechanism is: A. k [CO][Br2] B. k [CO] / [Br2]1/2 C. k[Br2] D. k [CO]2[Br2] E. k [CO][Br2]3/2

Consider the following reaction and its equilibrium constant: I2(g) + Br2(g) 2 IBr(g) Kc = 1.1...

Consider the following reaction and its equilibrium constant: I2(g) + Br2(g) 2 IBr(g) Kc = 1.1 × 102 This reaction mixture contains initially 0.41 M I2 and 0.27 M Br2. Calculate the equilibrium concentration of I2, Br2, and IBr? Please help with this, Can I find a example similar to this anywhere. I can't figure out some of the parts of this problem.

Part A The following three-step mechanism has been proposed for the decomposition reaction, 2H2(g)+2NO(g)→2H2O(g)+N2(g)2H2(g)+2NO(g)→2H2O(g)+N2(g): Step 1...

Part A The following three-step mechanism has been proposed for the decomposition reaction, 2H2(g)+2NO(g)→2H2O(g)+N2(g)2H2(g)+2NO(g)→2H2O(g)+N2(g): Step 1 2NO(g)⇌N2O2(g)2NO(g)⇌N2O2(g) Step 2 H2(g)+N2O2(g)→H2O(g)+N2O(g)H2(g)+N2O2(g)→H2O(g)+N2O(g) Step 3 N2O(g)+H2(g)→N2(g)+H2O(g)N2O(g)+H2(g)→N2(g)+H2O(g) Determine the molecularity for each of the elementary steps in order. View Available Hint(s) The following three-step mechanism has been proposed for the decomposition reaction, : Step 1 Step 2 Step 3 Determine the molecularity for each of the elementary steps in order. unimolecular, unimolecular, unimolecular unimolecular, bimolecular, bimolecular unimolecular, bimolecular, unimolecular bimolecular, bimolecular, bimolecular Submit Part...

Consider the following equilibrium for which H = 16.48: 2 NOBr(g) Y--> 2 NO(g) + Br2(g)...

Consider the following equilibrium for which H = 16.48: 2 NOBr(g) Y--> 2 NO(g) + Br2(g) How will each of the following changes affect an equilibrium mixture of the 3 gases in this reaction? (a) NO is added to the system. (b) The reaction mixture is heated. (c) The volume of the reaction vessel is doubled. (d) A catalyst is added to the reaction mixture. (e) The total pressure of the system is increased by adding a noble gas. (f)...

Question