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Chemistry

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Apr 3, 2024

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Chemical Kinetics Name Chemical Kinetics (Rate of Reaction) Four major things affect the rate of a reaction: Concentration: More molecules = more collisions Collisions are necessary for reactions Physical State: Ability to mix reactants Solids can be grinded to increase surface area Liquids can be stirred Temperature: Increases the kinetic energy of molecules Need sufficient energy to react (Activation Energy) Catalysts: Typically lower the activation energy of reactions For the majority of this guided inquiry we are going to use a simulation program written by Linda Koch, Ron LeMaster, Trish Loeblein, and Kathy Perkins. The program can be found by following this link: https://phet.colorado.edu/en/simulation/reactions-and-rates
Reactions & Rates (1.07) Single Collision Pull back the knob. What happened? (Discuss with your partner(s) or to yourself) Click the “Reload Launcher” button and expand the two windows on the right side of the program by clicking the “+” button for the Separation View and the Energy View. Now release the knob from various distances. Indicate on the potential energy diagram when the reaction proceeds forward. Now click the Angled Shot option in the top right corner. Try launching from a different angle or two. Did the reaction proceed as before? Why do you think this was the outcome despite having enough energy for the reaction to proceed? Potential Energy Reaction Coordinate No. The molecules collided, but they didn’t exchange the B component. Because the reactants needed to be placed correctly for the forward reaction to occur, the reaction was prevented. For the reaction to be effective, A must react with B with the B-C bond.
Set the Choose a reaction option to the last preset chemical reaction that isn’t Design your own . Now Change the Launcher Options back to Straight Shot and release the knob. What happens to the translational speed of the molecules as the reaction goes forwards and backwards? (Hint: the effect will be easiest to observe at a low energy) Please explain why this occurs. When the reaction goes forward in an exothermic reaction, energy is released as products are formed from reactants. This release of energy increases the kinetic energy of the molecules, causing them to move faster. As a result, the translational speed of the molecules increases. when the reaction goes backward (in the reverse direction), energy is absorbed rather than released. This absorption of energy decreases the kinetic energy of the molecules, causing them to slow down. Therefore, the translational speed of the molecules decreases.
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