Domenica DiStasio March 18 2019 Experiment 3 Chemical Kinetics Determining the Rate Equation Objective The objective of this lab was to use chemical kinetics in order to measure the speed rate of a chemical reaction The reaction we were interested in was the reaction of potassium permanganate with oxalic acid For our specific trials we looked at how the concentration of different solutions KMnO4 H2C2O4 and H2O affected the rate of the reaction Data Collection Rate equation k KMnO4 x H2C2O4 y Rate D KMnO4 Dt KMnO4 final KMnO4 init tfinal tinitial Volume Table KMnO4 Exp 1 Exp 2 Exp 3 10 mL 5 mL 10 mL H2C2O4 H2O 20 mL 20 mL 10 mL 0 mL 5 mL 10 mL Calculations M of KMnO4 021 mol L M of H2C2O4 5 mol L Experiment 1 KMnO4 1L x 021 03L 007 M Rate 1 007M 175 6 s 3 98E 5Msec 1 H2C2O4 02L x 5M 03L 333M Rate 1 333M 175 6s 1 9E 3Msec 1 Experiment 2 KMnO4 005L x 021 03L 035 M Tria1 1 Time 175 s 245 s 309 s Trial 2 Time 174 s 275 s 299 s Trial 3 Time 178 s 260 s 304 s Average Time 175 6 s 260 s 304 s Rate 2 035M 260 s 1 3E 4 H2C2O4 02L x 5M 03L 333M Rate 2 333M 260 s 1 3E 3Msec 1 Experiment 3 KMnO4 01L x 021M 03L 007 M Rate 3 007M 304 s 2 3E 5 H2C2O4 01L x 5M 03L 166M Rate 3 166M 304 s 5 5E 4Msec 1 a Finding x KMnO4 Rate 1 Rate 2 3 98E 5 1 3E 4 0 007 0 035 x 0 306 0 2x Log 0 306 log 0 2 x X 0 736 1 b Finding y H2C2O4 Rate 1 Rate 3 3 98E 5 2 3E 5 0 333 0 166 y Log 1 73 log 2 01 y Y 78 1 c Overall reaction order 1 1 2 Rate k KMnO4 1 H2C2O4 1 d Solving for k using experiment one Rate k KMnO4 1 H2C2O4 1 3 98E 5 k 0 007 0 333 3 98E 5 0 0023 k 0 0023 0 0023 k 0 0173Lmol 1sec 1 e Rate of reaction KMnO4 0 015L x 0 021M 0 05L 0 0063M H2C2O4 0 03L x 0 5M 0 05L 0 3M Rate k KMnO4 1 H2C2O4 1 Rate 0 0173 0 0063 0 3 3 27E 5 M 1sec 1 Conclusion The order of the reaction with respect to KMnO4 was 1 the order of the reaction with respect to H2C2O4 was 1 so therefore the overall order of the reaction was 2 We found that k is equal to 0 0173Lmol 1sec 1and our rate is 3 27E 5 M 1sec 1 If you increase the concentration the rate of the reaction also increases In this lab there were many areas where there could have been an error in the data If the amounts of each solution were not exact then the time for each trial would have been thrown off which would then throw off the rate of our reaction Human error would have attributed to the percent error of this lab which we did not calculate but I imagine it would not be 0
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