CHM 101L M5 Factors Affecting Reaction Rates Lab Report

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Southern New Hampshire University *

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101L

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Chemistry

Date

Feb 20, 2024

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Factors Affecting Reaction Rates Student Name Date

1 Data Activity 1 Data Table 1: Calibration Trial Na 2 S 2 O 3 (drops) Reaction time (sec) 1 8 31.85 2 7 34.6 3 6 27.56 1. How many drops will be used in the remaining experiments? There drops will be used in the rest of the experiment. Activity 2 Data Table 2a. Effects of KI (I - ) Concentration Tri al KI (drop s) HCl (drop s) Starc h (drop s) H 2 O (drop s) Na 2 S 2 O 3 (drops ) H 2 O 2 (mL ) Tim e 1 (sec ) Time 2 (sec) Averag e time (T avg ) (sec) Rate (1/T avg ) 1 8 2 4 0 3 0.4 12.5 8 18.9 5 19.20 0.05 2 8 2 4 0 3 0.4 25.4 0 19.87 3 6 2 4 2 0.4 25.1 2 21.67 21.90 0.05 4 6 2 4 2 0.4 24.9 9 15.90 5 4 2 4 4 0.4 38.3 5 30.94 30.06 0.03 6 4 2 4 4 0.4 24.8 5 26.11 7 2 2 4 6 0.4 41.3 5 57.85 53.75 0.02 8 2 2 4 6 0.4 52.2 7 63.52 Data Table 2b. Effects of H 2 O 2 Concentration © 2016 Carolina Biological Supply Company

2 Tri al KI (drop s) HCl (drop s) Starc h (drop s) H 2 O (mL ) Na 2 S 2 O 3 (drops ) H 2 O 2 (mL ) Tim e 1 (sec ) Tim e 2 (sec ) Average time (T avg ) (sec) Rate (1/T avg ) 1 8 2 4 0 0.4 15.2 5 14.9 9 15.57 0.05 2 8 2 4 0 0.4 15.1 2 16.9 7 3 8 2 4 0.1 0.3 19.8 3 25.2 0 22.05 0.06 4 8 2 4 0.1 0.3 21.5 7 21.5 6 5 8 2 4 0.2 0.2 24.8 9 30.9 3 27.66 0.05 6 8 2 4 0.2 0.2 26.8 9 27.9 1 7 8 2 4 0.3 0.1 50.9 1 59.9 4 52.10 0.02 8 8 2 4 0.3 0.1 52.5 1 44.9 1 Data Table 2c. Effects of HCl (H + ) Concentration Tri al KI (drop s) HCl (%) Starc h (drop s) H 2 O (drop s) Na 2 S 2 O 3 (drops ) H 2 O 2 (mL ) Tim e 1 (sec ) Tim e 2 (sec ) Average time (T avg ) (sec) Rate (1/T avg ) 1 8 100 % 4 0 0.4 15.9 9 14.7 0 15.62 0.06 2 8 100 % 4 0 0.4 16.2 2 15.5 7 3 8 75% 4 0 0.4 18.7 1 17.8 5 18.55 0.05 4 8 75% 4 0 0.4 18.1 2 19.5 4 5 8 50% 4 0 0.4 15.3 8 14.5 3 15.11 0.07 6 8 50% 4 0 0.4 16.4 0 14.1 1 7 8 25% 4 0 0.4 23.5 1 25.6 7 24.02 0.04 8 8 25% 4 0 0.4 23.0 0 23.8 9 Activity 3 © 2016 Carolina Biological Supply Company

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3 Data Table 3. Temperature Effects Water bath trial Temperature of the water bath (°C) Reaction time (sec) Cold water 5 60.97 Room-temperature water 24 17.02 Hot water 45 7.95 2. Explain how each of these treatments affected the reaction rate. Describe the effect at a molecular level. a. Concentration The degree of concentration of reactant determines how close they may be. This state of affairs will make them more likely to collide. Consequently, this will intensify the reaction rate. At this rate, it will take less time for atoms to bump and collide. b. Temperature Higher temperature correlates with the vigorous movement of the atoms in the substance. At this rate, the atoms will move faster and collide; hence generating the right reaction. Activity 4 Data Table 4. Catalyst Trial Water (drops) CuSO 4 (drops) Reaction time (sec) 1 4 0 47.93 2 3 1 38.24 3 2 2 32.08 4 1 3 27.27 5 0 4 18.85 3. How did the addition of copper (II) sulfate affect the reaction rate? Did the amount of catalyst affect the reaction rate? The addition of copper (II) sulfate unquestionably increased the reaction rate. As the drops of copper (II) sulfate increased, the reaction rate became shorter. Catalyst has its effect as well, which is increase further the reaction rate. © 2016 Carolina Biological Supply Company

4 Activity 5: Data Table 5. Orders of Reactants in the Rate Law R = k [I – ] m [H 2 O 2 ] n [H + ] p Calculated Reaction order (X) (e.g. ( concentration 1 concentration 2 ) X = rate 1 rate 2 ) Reactan t Concentrati on Averag e Rate Calculated Reaction order (X) Averag e Reactio n order Reactio n Order (integer ) KI (I  ) 8 drops 0.05 0.61493 79 m = 1 0 KI (I  ) 6 drops 0.05 1.25985101 KI (I  ) 4 drops 0.03 0.58496251 KI (I  ) 2 drops 0.02 H 2 O 2 0.4 mL 0.06 0.72803 35 n = 1 0.63376059 H 2 O 2 0.3 mL 0.05 0.55033972 H 2 O 2 0.2 mL 0.04 1 H 2 O 2 0.1 mL 0.02 HCl (H + ) 100% 0.06 0.20375 753 p = 0 0.63376059 HCl (H + ) 75% 0.05 -0.82984265 HCl (H + ) 50% HCl (H + ) 25% Rate law R=548[I-][H2O2] © 2016 Carolina Biological Supply Company

5 Reactan t Concentrati on Averag e Rate Calculated Reaction order (X) Averag e Reactio n order Reactio n Order (integer ) Overall order of the reaction 2 4. Use the rate-law expression you determined for Data Table 5 to answer the following questions. a. If the concentration of I – was doubled, how would that affect the reaction rate? According to the given rate law expression, the reaction rate is directly proportional to the concentration of iodide ions [I-]. If the concentration of I- is doubled, the reaction rate would also double, provided that the concentrations of other reactants remain constant. b. If the concentration of H 2 O 2 was halved, how would that affect the reaction rate? The reaction rate would not increase but decrease by a factor of 2. The rate of reaction is proportional to the concentration of HO ₂ . c. If the concentrations of I – and H 2 O 2 were both doubled, how would that affect the reaction rate? The rate doubles when the concentration is doubled. The rate is related to the square of a reactant's concentration. d. If the concentration of H + (HCl) was doubled, how would that affect the reaction rate? The reaction rate would not be affected if the concentration of H (HCl) was doubled. © 2016 Carolina Biological Supply Company

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