Laboratory 7: Activation Energy Determination Name: Averie Hayes Date:03/08/21 Objective: The overall objective of this experiment is to determine the activation energy of a chemical reaction that will occur in this lab. Procedure 1: (Record every 10 seconds) 1. Place the room temperature 4.0 mL 3% H2O2 into the container, then the container into the water bath. 2. Measure and record bath temperature 3. Add room temperature 1.0 mL 0.50 M KI solution from ice bath to reaction container, leave container in bath 4. Stopper the reaction container and record pressure data 5. Record temperature data and pressure data in Table 1 Procedure 2: (Record every 20 seconds) 1. Place water beaker with 300 mL of water on hot plate at medium setting 2. Place 4.0 mL 3% H2O2 of cooled solution into reaction container, then into ice bath 3. Record data 4. Add 1.0 mL 0.50 M KI into reaction container and leave in ice bath 5. Stopper container and record pressure data 6. Record in Table 3 Procedure 3: (Record every 5 seconds) 1. Once the water on the hot plate is heated, place an aliquot of 4.0 mL 3% H2O2 and an aliquot of 1.0 mL 0.50 M KI in into the warm water 2. Place water beaker with 300 mL of water on hot plate at medium setting 3. Place 4.0 mL 3% H2O2 of cooled solution into reaction container, then into warm water bath 4. Record data 15. Add 1.0 mL 0.50 M KI into reaction container and leave in ice bath 6. Stopper container and record pressure data 7. Record in Table 4 Data and Calculations: Table 1. Concentration and Initial Rate Data Table 2: Table 3: Table 4: 2 Procedure (Temp,K) [H2O2]M [KI]M Rate (atm/s) Rate Constant 1(293.85K) .88 0.5 .0005 .011 2(276.75) .88 0.5 -.0001 -.0002 3(312.95) .88 0.5 .0013 .0029Graph 2: Graph 3: 3Graph 4: Answers to Key Questions: 1. What do the equations above suggest about the order of reaction with respect to each reactant? They are both of the first order. 2. What is the overall order of reaction based on the equations above? 2 3. Why is there no sign in front of the the change in oxygen pressure as a function of the change in time? Oxygen increases as the reaction occurs, because it is a product of the reaction, therefore there is no sign because it is a positive value. 44. What should be the effect on the rate constant k by decreasing the temperature of a reaction? Decreasing the temperature should decrease the rate of reaction 5. What should be the effect on the reaction rate by decreasing the temperature of a reaction? By decreasing the temperature, you decrease the rate of reaction,k, which will slow down the reaction overall. 6. Should the A term in the Arrhenius equation be affected by changes in temperature? Yes, but it is considered constant within a small range of temperatures 7. Which term of the linearized Arrhenius equation represents the y-value? lnK 8. Which term of the linearized Arrhenius equation represents the x-value? (1/T) 9. Which term of the linearized Arrhenius equation represents the slope, m? -(Ea/R) 10. Which term of the linearized Arrhenius equation represents the intercept, b? lnA 11. Determine the activation energy and the frequency factor for the KI catalyzed decomposition reaction of H2O2. Activation Energy=-R*Slope -(.008314 kJ mol*K)x(-.0001)= .0000008314kJ-mol A= (b=.0027)(lnA=.0027) A is equal to e^lnA so A=1.003 5Conclusion: Overall this lab helped us to learn how to determine the activation energy of a chemical reaction, given the concentrations and initial rates of said reaction.