Homework Answers
As higher the value of k , then step is faster hence it has lowest activation energy and lower the value of k , slower the step hence higher the activation energy.
K3>K1>K2 and order of activation energy
Ea2 > Ea1>Ea3
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23. The mechanism for the endothermic reaction [2A + C + D + F) is shown...
3. A reaction 2A 2B + C is known to follow second-order kinetics, with k =...
3. A reaction 2A 2B + C is known to follow second-order kinetics, with k = 7.20x10*M's' at 25.0 °C. (20 points) During one experiment, the initial concentration of A is [A]. = 0.120 M (a) Calculate the half-life (1,2), in hours, for this experiment. (b) Calculate the initial reaction rate (in M/s) for this reaction (4 points) (c) How long will it take (in hours) for the concentration of C to reach [C] = 0.0540 M (6 points) (d)...
5. For the overall exothermic reaction: H2(g) + Br2(g) → 2HBr(g) the following mechanism was determined:...
5. For the overall exothermic reaction: H2(g) + Br2(g) → 2HBr(g) the following mechanism was determined: fast Equilibrium Step 1: Brz(8) 2Br(g) Step 2: H2(g) + Br(g)_52HBr(g) + H(g) Step 3: H(g) + Br(g) k3 HBr(g) slow fast Use a plot of AH versus Reaction Pathway to illustrate the three step reaction profile.
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.
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?...
A chemical reaction, A+B → P, has the following mechanism: 2A< Ki>A, (fast to equilibrium) A+B&K, ™C (fast to...
A chemical reaction, A+B → P, has the following mechanism: 2A< Ki>A, (fast to equilibrium) A+B&K, ™C (fast to equilibrium), A,+C-k>P+ 2A (slow) where Kį and K2 are the equilibrium constants for the first two reactions, respectively. k3 is the rate constant for the third reaction. (a) [5 points] Based on this mechanism, show that the rate of product (P) formation is: d[P] – k[A[B], where k is the rate constant of the overall reaction. Write k in terms of...
Credit for work. Thank you 14 14) (a) For the reaction of CH) + C&H) -...
Credit for work. Thank you
14 14) (a) For the reaction of CH) + C&H) - CH10. The activation energy (E.) for the forward readtion is 115 kJ/mol, and the activation for the reverse reaction (decomposition of cyclohexene to ethylene and butadiene) is 287 mol. Draw the energy diagram (potential energy versus progress of the reaction) (b) Calculate the heat of reaction, a H . for the forward reaction Show it on the graph. Is the reaction endothermic or exothermic?...
8. (20 points) Consider the following mechanism, with the accompanying energy diagram, which has been suggested...
8. (20 points) Consider the following mechanism, with the accompanying energy diagram, which has been suggested for the following overall reaction in the presence of a Cl catalyst: 03 +0 202 Step 1: Step 2: 03 + Cl → OCl + O2 OCl + 0 + 02 + Cl +---Ea, Energy - - - - AHrxn --- - Reaction progress- A. Based on the energy diagram, which step is rate limiting? Which step is the fastest? (4 Points) B. Identify...
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?...
3—Part II: For the following hypothetical mechanism Step (1) slow 2 A+ E + C +...
3—Part II: For the following hypothetical mechanism Step (1) slow 2 A+ E + C + F Ea = 40 kJ, AH = + 15 kJ Step (2) fast 3 B+F → D+E Ea = 15 kJ, AH = -20 kJ Draw the energy diagram for this 2-step mechanism. Label all parts of the diagram and locate (i.e. indicate) all energy values on your diagram. Calculate the overall enthalpy change for this reaction. Note: must set scale & honour proportionality.
For the first-order reaction X ⟶ products, which of the following graphs is best for determining...
For the first-order reaction X ⟶ products, which of the following graphs is best for determining the activation energy, Ea ? Note: The best choice is the one that yields a straight line graph with the slope directly proportional to Ea . In the options below, T is the kelvin temperature and t is time. (a) k versus 1/T (b) 1 / [X] versus t (c) ln k versus T (d) ln [X] versus t (e) [X] versus t (f)...
3. A reaction 2A 2B + C is known to follow second-order kinetics, with k = 7.20x10*M's' at 25.0 °C. (20 points) During one experiment, the initial concentration of A is [A]. = 0.120 M (a) Calculate the half-life (1,2), in hours, for this experiment. (b) Calculate the initial reaction rate (in M/s) for this reaction (4 points) (c) How long will it take (in hours) for the concentration of C to reach [C] = 0.0540 M (6 points) (d)...
5. For the overall exothermic reaction: H2(g) + Br2(g) → 2HBr(g) the following mechanism was determined: fast Equilibrium Step 1: Brz(8) 2Br(g) Step 2: H2(g) + Br(g)_52HBr(g) + H(g) Step 3: H(g) + Br(g) k3 HBr(g) slow fast Use a plot of AH versus Reaction Pathway to illustrate the three step reaction profile.
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?...
A chemical reaction, A+B → P, has the following mechanism: 2A< Ki>A, (fast to equilibrium) A+B&K, ™C (fast to equilibrium), A,+C-k>P+ 2A (slow) where Kį and K2 are the equilibrium constants for the first two reactions, respectively. k3 is the rate constant for the third reaction. (a) [5 points] Based on this mechanism, show that the rate of product (P) formation is: d[P] – k[A[B], where k is the rate constant of the overall reaction. Write k in terms of...
Credit for work. Thank you
14 14) (a) For the reaction of CH) + C&H) - CH10. The activation energy (E.) for the forward readtion is 115 kJ/mol, and the activation for the reverse reaction (decomposition of cyclohexene to ethylene and butadiene) is 287 mol. Draw the energy diagram (potential energy versus progress of the reaction) (b) Calculate the heat of reaction, a H . for the forward reaction Show it on the graph. Is the reaction endothermic or exothermic?...
8. (20 points) Consider the following mechanism, with the accompanying energy diagram, which has been suggested for the following overall reaction in the presence of a Cl catalyst: 03 +0 202 Step 1: Step 2: 03 + Cl → OCl + O2 OCl + 0 + 02 + Cl +---Ea, Energy - - - - AHrxn --- - Reaction progress- A. Based on the energy diagram, which step is rate limiting? Which step is the fastest? (4 Points) B. Identify...
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?...
3—Part II: For the following hypothetical mechanism Step (1) slow 2 A+ E + C + F Ea = 40 kJ, AH = + 15 kJ Step (2) fast 3 B+F → D+E Ea = 15 kJ, AH = -20 kJ Draw the energy diagram for this 2-step mechanism. Label all parts of the diagram and locate (i.e. indicate) all energy values on your diagram. Calculate the overall enthalpy change for this reaction. Note: must set scale & honour proportionality.
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