A gaseous reaction occurs by a two-step mechanism, shown
below.
Step 1: A2 ⇄ 2 A fast
Step 2: A + B → AB slow
Which is the rate of the reaction?
A gaseous reaction occurs by a two-step mechanism, shown below. Step 1: A2 ⇄ 2 A ...
An endothermic aqueous reaction occurs by a two-step mechanism, shown below. Step 1: A2X2 +Y---> A2X +XY (slow) Step 2: A2X2 +XY --->A2X + X2 + Y (fast) -write the overall reaction. -In this reaction the intermediate is _____, and the catalyst is _____. -Sketch the reaction profile for the overall uncatalyzed reaction. -On the same graph sketch the reaction profile for the catalyzed reaction.
Suppose the reaction: A + 2B - AB2 occurs by the following mechanism: Step 1 A + B - AB slow Step 2AB + B - AB fast The rate law expression for the reaction is
For a reaction that proceeds by the following two-step mechanism A2 ⇄ 2A (fast) A + B → C (slow) Which of the following statements is/are correct? 1) The reaction is first order in the concentration of A2. 2) B is a reaction intermediate. 3) The rate-determining step is bimolecular. 4) The units of the specific rate constant are mol1/2L-1/2s-1
8. (2 points) Consider the mechanism below Step 1 (slow) A2 BC AB+AC AB BC B2AC Step 2 (fast) B2+ 2 AC overall A22 BC What is the rate law of the reaction? a. b. What compound is considered an intermediate?
Predict the overall reaction from the following two-step mechanism: 2 A→A 2(fast) A2+B→A2B(slow) Express your answer as a chemical equation. Predict the rate law from the following two-step mechanism: 2A⇌ A2 (fast) A2+B→A2B (slow)
Question 4 of 10 For a reaction that proceeds by the following two-step mechanism A2 =2A (fast) A+B-C (slow) Which of the following statements is/are correct? 1) The reaction is first order in the concentration of Az. 2) B is a reaction intermediate. 3) The rate-determining step is bimolecular. 4) The units of the specific rate constant are mol1/2_-1/2-1 O A. 1 & 3 only B. 2 only C. 3 only OD. 1 & 4 only O E.2 & 3...
An aqueous reaction occurs by a two-step mechanism, shown below. Step 1: A2X2 + Y → A2X + XY Step 2: A2X2 + XY → A2X + X2 + Y In this reaction the intermediate is ________, and the catalyst is ________.
4. Below is a proposed mechanism for a reaction: Step 1. Step 2. C+E-F Step 3. F G A B C+D Fast equilibrium Slow Fast A. (2 points) What is the overall stoichiometry for this reaction? B. (2 points) Which step is the rate determining step? C. (6 points) If this mechanism is correct, what should the rate equation for this reaction be? (Make sure you include the fast equilibrium)
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...
The rate law for the mechanism below is A2(g) ⇌ 2A(g) K1, fast A(g) + B(g) ⇌ AB(g) K2, fast AB(g) + A(g) → A2B(g) k3, slow Options: rate = K2k3[A]2[B] rate = K1K2k3 [A2][B] rate = K10.5k3 [A2]0.5[AB] rate = k3[A][AB] rate = K10.5K2k3 [A2]0.5[A] [B]