Mechanism 1 Mechanism 2 Mechanism 3 10. Three different mechanisms are A+Y C+D slow B+C E+Y fast A → Q+D sk B+Q→ E A+B > F slow proposed for an exothermic reaction, shown here: → D+E fast F fa a)What is the overall reaction? (in box) b)Circle any intermediates(s) in these mechanisms. c)Put a box around any catalyst(s) in these mechanisms. d)Do any of these mechanisms have a second order rate law? If yes, circle here: Mech 1 Mech 2 Mech 3

Mechanism 1 Mechanism 2 Mechanism 3 10. Three different mechanisms are A+Y C+D slow B+C E+Y fast A → Q+D sk B+Q→ E A+B > F slow proposed for an exothermic reaction, shown here: → D+E fast F fa a)What is the overall reaction? (in box) b)Circle any intermediates(s) in these mechanisms. c)Put a box around any catalyst(s) in these mechanisms. d)Do any of these mechanisms have a second order rate law? If yes, circle here: Mech 1 Mech 2 Mech 3

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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6. Given the reaction: CH3(CO)CH3 (M) | B(M) 0.010 0.010 CH3(CO)CH3 + I2 + H* → CH3(CO)CH2I + HI H* (M) Rate (M/s) 0.010 3.0 x 10-4 0.010 6.0 x 10-4 0.020 6.0 x 104 0.020 2.4 x 10-3 0.040 4.8 x 10-3 0.010 6.0 x 104 0.010 0.020 0.010 0.040 0.040 0.020 0.020 0.040 0.020 0.040 a. Determine the reaction order for each reactant. b. Solve for the rate constant, k, and the appropriate units. c. Write the rate law for the reaction, including a value for k. d. Solve for the rate of the reaction if there are 1.25 M of CH3(CO)CH3, 2.25 M of I2, and 3.25 M H*.
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= For a different reaction X2Y, the initial [X] 1.0 M, and [Y] = 0 M. After 5 minutes the [X] has fallen to 0.8 M and then does not change any further. Draw a graph of [X] v time for the first 10 minutes. Use the blank template graph from Q1. Use the editor to format your answer
2 NO(g) + Br2 (g) → 2 NOB1(g) Initial Rate Experiment NO] (M) [Br2] (M) (mol/L's) 1 1.0 x 10-2 2.0 × 10-2 2.4 x 10-2 2 4.0 x 10-2 2.0 × 10-2 0.384 3 1.0 x 10-2 6.0 x 10-2 7.2 x 10-2 What is the order of the reaction with respect to [NO] and [Br2], and what is the overall order of the reaction? Order with respect to [NO] = Order with respect to [Br2] = Overall order
Identify the catalyst and the intermediate in the following reaction mechanism Cl + 03 > CIO + 02 Cio + 0> Cl + 02 Overall reaction for mechanism The catalyst in the above reaction mechanism is because The intermediate in the above reaction mechanism is _ because Do the catalyst or the intermediate appear in the overall reaction? How can you tell a catalyst apart from an intermediate in a reaction mechanism?
10. Which mechanism is going to produce a faster reaction? Explain. Mechanism 2 Mechanism 1 STEP 1 NO + 03 → NO2 + 02 STEP 1 STEP 2 03 02 +0 03 +0 202 STEP 2 - 02 +0 NO2 +0 NO + 02 03 STEP 3 OVERALL 203 → 302 OVERALL 203 → 302
please answer both please i will upvote ( if you have plan to answer only one then please skip , let someone accept the question who can do both )
Consider this three-step mechanism for a reaction: Cl₂ (g) Cl(g) + CHCl3 (g) Cl(g) + CCl3 (g) k₂ → k3 → k4 2Cl(g) (fast) HCl(g) + CCl3(g) (slow) CCl4 (g) (fast)
Reaction to produce COCl2 (phosgene) from chlorine and carbon monoxide in a gaseous stateIt is said that the mechanism of is as follows.1st step: Cl2 ⇔ 2 Cl (Fast equilibrium)2nd step: Cl + CO ⇔ COCl (Fast equilibrium)3rd step: COCl + Cl2 ⇒ COCl2 + Cl (slow)4th step: 2 Cl ⇒ Cl2 (fast)Overall reaction: CO + Cl2 ⇒ COCl2Derive the rate law of this reaction.
This question has multiple parts. Work all the parts to get the most points. The reaction 2NO(g) + Cl₂ (g) → 2NOCI(g) was studied at -10°C. The following results were obtained where A[C1₂] At Rate = [NO], [C12]o (mol/L) (mol/L) 0.12 0.12 0.12 0.24 0.24 0.24 Initial Rate (mol/L.min) 0.31 0.62 2.49 a What is the rate law? (Use k for the rate constant. ) Rate = k[NO]²[C1₂] b What is the value of the rate constant? Rate constant = L² mol². min
Analyze the following reaction mechanism: 1. H₂O2 → H₂O + O 2. O + CF₂Cl2 → CIO + CF₂CI 3. CIO + O3 → CI + 20₂2 4. CI+ CF₂CI → CF₂Cl2 Identify the reaction intermediates in this reaction. A) O, CIO, CI B) CI, CF₂CI, CF₂Cl2 C) O, CIO, O, H₂O D) O, CIO, CI, CF₂CI E) O, CIO, CI, CF₂Cl2 ULL