Sketch an energy level diagram for this overall reaction, which is exothermic. Add to your diagram a second sketch for the uncatalyzed reaction. Clearly label which curve is catalyzed, and which is uncatalyzed. Also label the activation energy (EA) and the AH for each reaction. Use your diagram to explain why one of these reactions is faster than the other, even though they start and end in the same place.

Sketch an energy level diagram for this overall reaction, which is exothermic. Add to your diagram a second sketch for the uncatalyzed reaction. Clearly label which curve is catalyzed, and which is uncatalyzed. Also label the activation energy (EA) and the AH for each reaction. Use your diagram to explain why one of these reactions is faster than the other, even though they start and end in the same place.

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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opy of reaction 4. When a lit match is touched to the wick of a candle, the candie begins to burn. When the match is removed, the candle continues to burn, what is the role of the match? A. behaves as a catalyst B. supplies the activation energy C. is part of the rate determining step D. lowers the activation energy barrier 5. How does a catalyst increase the rate of a reaction? A. increasing the concentration of reactant(s) B. decreasing the concentration of the reactant(s) C. increasing the activation energy of the overall reaction D. decreasing the activation energy of the overall reaction 6. Which of the following would NOT increase the rate of reaction. A. adding catalyst B. raising the temperature. C. increasing the volume of the container D. increasing the concentration of the reactants 7. Why do dust particles suspended in the air inside unheated grain elevators can sometimes react explosively? It is because the dust particles have A. high kinetic energy B. high activation…
Classify the actions based on how they could affect a reaction rate. Rate increases Rate decreases Rate is unaffected Answer Bank decrease the concentration of a reactant decrease the surface area of a solid reactant increase the temperature add a catalyst
The rate of a reaction is how quickly the reaction goes to completion. If two reactions have the same amount of reactant, increasing the rate does not increase the amount of product produced, it simply reduces the time that it takes to make the product. Using the internet , research the one factors below that affect the rate of a chemical reaction. 1. Reactant concentration ( add an example and be very detailed add graphs as well) Be sure to include the following terms as they relate to chemical reactions: collision theory Be very detailed potential energy diagrams be very detailed activation energy be very detailed Your work should be written in complete sentences, and assume your audience is grade 11 chemistry students who do not understand this unit. Make sure all research is put into your own words!
Consider this reaction: Br CH₂OH + Br-Br H₂CO The mechanism proceeds through a first cationic intermediate, intermediate 1. Nucleophilic attack leads to intermediate 2, which goes on to form final product. In cases that involve a negatively charged nucleophile, the attack of the nucleophile leads directly to the product. Year Hot Br + CH₂OH Br Intermediate 1 Intermediate 2 (product) In a similar fashion, draw intermediate 1 and intermediate 2 (final product) for the following reaction. Br H Br₂ + NaBr + H2O H H H NaOH . Pay attention to the reactants, they may differ from the examples. In some reactions, one part of the molecule acts as the nucleophile. Structures are provided for you to modify in the sketchers below. . • You do not have to consider stereochemistry. • Draw one structure per sketcher. Add additional sketchers using the drop-down menu in the bottom right corner. Separate intermediate 1 and intermediate 2 using the symbol from the dropdown menu. Sn [F H On [F I Br -OH HH…
Explain in your own words and develop the reaction mechanism.
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11. Draw a potential energy diagram for a two-step reaction in which the activation energies are 10 kcal/mol (first step) and 3 kcal/mole (second step), the intermediate is 5 kcal/mol higher in energy than the reactants, and the products are 1 kcal/mol lower in energy than the reactants. Label both axes and positions on the curve that correspond to reactants (R), the intermediate (I), transition states (TS₁, TS₂), and products (P). Indicate the activation barriers with vertical lines and the labels Ea1 and Ea2.
1. a. Explain in your own words, what is meant by the term "activation energy." b. How can the idea of activation energy be used to explain the temperature dependance of rate? c. How can activation energy be used to explain why a catalyst increases the rate of a chemical reaction
The rate of a reaction is how quickly the reaction goes to completion. If two reactions have the same amount of reactant, increasing the rate does not increase the amount of product produced, it simply reduces the time that it takes to make the product. Using the internet, research the Reactant concentration factor below that affect the rate of a chemical reaction. 1. Reactant concentration (be very detailed add graphs to explain your details it should be 300 words) Your work should be written in complete sentences, and assume your audience is grade 11 chemistry students who do not understand this unit. Make sure all research is put into your own words!
400 300 + energy 200 - (kJ/mol) с +D 100 A + В reaction coordinate Use the energy diagram to answer these questions. I KJ/mol What is the heat of reaction? Exothermic Is the reaction exothermic or endothermic? Endothermic Neither Yes, it's kJ/mol Can you determine the activation energy? No. Can you determine the activation energy of the reverse reaction? Yes, it's kJ/mol С+D- A+B No.
Comment how the temperature affects the rate. a. Temperature definitely has an affect on the rate. When there is an increase in temperature, the rate at which the reaction occurs also increases. This is proved through my data. As each experiment had an increasing temperature, here are my rates that go from lowest to highest temperature: 3.25*10 M/s, 4.15*10 M/s, 6.85*10 M/s, 9.17*10* M/s. With this increase in temperature, there is therefore an increase in the energy of molecules in the solution. With this increase in energy, there is an increase in collisions with enough energy, and this ultimately leads to the rate increasing.
10.a. A student performed the following kinetic isotope effect experiment. • The reaction below took 15 min to achieve completion. H3C H3C HI Br D3C • The reaction below (note deuterium replacement) took 60 min to achieve completion. CD3 D3C D H Br This group is isopropyl, going backwards into paper NaOEt EtOH -CD3 NaOEt EtOH D Draw the correct mechanism(s) and product(s) for the top reaction with H-labeled reactant. Show stereochemistry clearly.