Reaction Coordinate Diagrams & Catalysts Prachi Patel

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Purdue University *

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112

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Chemistry

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Dec 6, 2023

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Activities and Explorations: 10 points, Due Sunday, April 9, 11:59 PM Kinetics, Reaction Coordinate Diagrams, Catalysts Instructions: Upload your work on this page to Brightspace by typing or writing your responses and saving the file and uploading that file as a pdf. You can also take pictures of your written work and paste them into this document and save is as a pdf. Learning Objectives 13.4 Activation Energy and Temperature Dependence of Rate Constants • Identify activation energy on a Potential Energy versus Reaction progress graph. 13.6 Catalysis • Define catalyst and how it impacts the rate of a chemical reaction using both words and Potential Energy versus Reaction progress graphs. • Differentiate between a catalyzed and uncatalyzed reaction using a Potential Energy versus Reaction progress graph. Instructions : Answer the questions below. Be sure to show your work using mathematical calculations of drawings, as appropriate. Upload your file as a pdf into Brightspace when you are finished. Three reaction coordinate diagrams are included below. Each diagram represents a different chemical reaction (Reactions 1 – 3). Dashes lines are included to show that the potential energy axes are comparable across all three diagrams. 1. (1 pt) What significant differences can you identify between the three reaction coordinate diagrams? List at least two differences you can find. Feel free to draw on the graphs if that would help! For reaction three the activation energy is lower than the activation energy for reaction 1 and reaction 2. For reaction 1 and 3, the transition from reactants to products is a little bit broader than reaction 2. 2. (1 pt) How do the rates of Reactions 1, 2, and 3 compare to one another? Use language such as “less than,” “greater than,” or “equal to” in your comparison. The rate of reaction for reaction 3 is greater than the rate reaction for reaction 2. The rate of reaction for reaction 2 is greater than the rate of reaction for reaction 1.
3. (2 pts) Explain your answer to #2. Use specific evidence from the diagrams in question #1 in your explanation. Lowest activation energy means the highest rate of reaction; that is why reaction 3 has the highest rate of reaction. Reaction 1 and 2 have the same activation energy, but reaction 1 is broader than 2. If the reaction is broader can mean that there will be a higher probability that the reactants will go back to the reactant state than going to the product state. The probability is less likely for two because it is less broad, so reaction 2 will have the highest reaction rate and reaction 1 will have the lowest reaction rate. 4. A reaction diagram is shown at right for the reaction A B. a. (2 pt) How would the diagram change if a catalyst was present? Explain in words and show what the new reaction diagram would look like on the graph by directly drawing on it . The slope of the activation energy will be lower after the addition of a catalyst. b. (1 pt) Exactly what does a catalyst do to change the the rate of the reaction? (Assume the temperature does not change.) A catalyst speeds up a reaction by lowering the activation energy. It speeds up the reaction without being consumed by the reaction. 5. (3 pts) Consider the graphs below for the reactions A and B and fill in the table. Reaction A Reaction B
Determine the activation energy and H for each reaction and whether the reaction is exothermic or endothermic. Reaction A Reaction B Activation Energy (kJ) 50 300 H (kJ) 100 200 Exothermic or Endothermic e xothermic e ndothermic
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