An endothermic aqueous reaction occurs by a two-step mechanism, shown below. Step 1: A2X2 +Y---> A2X...
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.
Homework Answers
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An endothermic aqueous reaction occurs by a two-step mechanism,
shown below.
Step 1: A2X2 +Y---> A2X...
An aqueous reaction occurs by a two-step mechanism, shown below. Step 1: A2X2 + Y →...
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 ________.
A gaseous reaction occurs by a two-step mechanism, shown below. Step 1: A2 ⇄ 2 A ...
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?
Can you please answer the following questions? The rate constant, k for the reaction below A...
Can you please answer the following questions?
The rate constant, k for the reaction below A - Products is 2.8 x 10 sat 80°C. If the initial concentration of A is 0.25M, what is the concentration after 50 s? The oxidation reaction of thallium (I) by cerium (IV) is believed to occur via three steps. The rate low for the reaction is: rate = k[Ce [Mn2") ce". Mne - Cen ! ce". Mn. Cell. Mn TI". Mn* - TI. Mn?...
2. Consider this two step mechanism for a reaction… Step 1 NO2 + O3 --> NO3 ...
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...
6. The decomposition of ozone in the upper atmosphere is catalyzed by NO. The overall reaction...
6. The decomposition of ozone in the upper atmosphere is catalyzed by NO. The overall reaction and rate law are: O:(g) + O(g) →202(g): rate = k[O][NOJ Write a possible mechanism that is consistent with rate law and identify an intermediate in the reaction. 7. A possible mechanism for the iodide ion catalyzed decomposition of hydrogen peroxide in aqueous solution is: H2O2(aq) + I'(aq) → H2O(l) + Of(aq) ---...-slow H2O2(aq) + Or(aq) → H2O(0) + O2(g) + I'(aq) -----fast What...
Suppose a reaction occurs with the following mechanism: Step 1: 2AD Step 2: D+E- (fast) B+C...
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...
Suppose the reaction: A + 2B - AB2 occurs by the following mechanism: Step 1 A...
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
11. Below are 2 possible reaction mechanisms (pathways) for the reaction Mechanism 1 No, + 03...
11. Below are 2 possible reaction mechanisms (pathways) for the reaction Mechanism 1 No, + 03 → No, (fast) NOs + NOs → N20s + 5/202 (slow) Mechanism 2 NO2 + 03 → NO3 + 02 (slow) No, + NO2 → N20s (fast) If the reaction rate law is found to be: rate = k[NO21 Which mechanism is consistent with this rate law (1 or 2) What is/are the intermediate/s for Mechanism 1? What is/are the intermediate/s for Mechanism 2?...
4. Below is a proposed mechanism for a reaction: Step 1. Step 2. C+E-F Step 3....
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)
1. Write a rate law from the image below: TRANSITION STATES Ea(step 2) Ea(step 1) slow...
1. Write a rate law from the image below: TRANSITION STATES Ea(step 2) Ea(step 1) slow fast Potential energy NO2F+ F+NO2 2NO2 + F2 REACTANTS ΔΗ 'nxn <0 2NO2F PRODUCT Reaction progress A. Rate = k [NO2] B. Rate = k [NO2][F2] C. Rate = k [NO212[F2] 2. What is the overall reaction? A. 2 NO2 + F2 → 2 NO2F B. NO2 + F2 → NO2F +F + NO2 C. NO2 + F2 → 2 NO2F 3. Write out...
Can you please answer the following questions?
The rate constant, k for the reaction below A - Products is 2.8 x 10 sat 80°C. If the initial concentration of A is 0.25M, what is the concentration after 50 s? The oxidation reaction of thallium (I) by cerium (IV) is believed to occur via three steps. The rate low for the reaction is: rate = k[Ce [Mn2") ce". Mne - Cen ! ce". Mn. Cell. Mn TI". Mn* - TI. Mn?...
6. The decomposition of ozone in the upper atmosphere is catalyzed by NO. The overall reaction and rate law are: O:(g) + O(g) →202(g): rate = k[O][NOJ Write a possible mechanism that is consistent with rate law and identify an intermediate in the reaction. 7. A possible mechanism for the iodide ion catalyzed decomposition of hydrogen peroxide in aqueous solution is: H2O2(aq) + I'(aq) → H2O(l) + Of(aq) ---...-slow H2O2(aq) + Or(aq) → H2O(0) + O2(g) + I'(aq) -----fast What...
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...
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
11. Below are 2 possible reaction mechanisms (pathways) for the reaction Mechanism 1 No, + 03 → No, (fast) NOs + NOs → N20s + 5/202 (slow) Mechanism 2 NO2 + 03 → NO3 + 02 (slow) No, + NO2 → N20s (fast) If the reaction rate law is found to be: rate = k[NO21 Which mechanism is consistent with this rate law (1 or 2) What is/are the intermediate/s for Mechanism 1? What is/are the intermediate/s for Mechanism 2?...
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)
1. Write a rate law from the image below: TRANSITION STATES Ea(step 2) Ea(step 1) slow fast Potential energy NO2F+ F+NO2 2NO2 + F2 REACTANTS ΔΗ 'nxn <0 2NO2F PRODUCT Reaction progress A. Rate = k [NO2] B. Rate = k [NO2][F2] C. Rate = k [NO212[F2] 2. What is the overall reaction? A. 2 NO2 + F2 → 2 NO2F B. NO2 + F2 → NO2F +F + NO2 C. NO2 + F2 → 2 NO2F 3. Write out...
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