Calculate the value of the rate constant for each run and calculate the average value. Indicate the units for the rate costant. Given : Rate of reaction for run 1= 1.08 x10-6 M/sRate law for Run 1 : 1.08 x10-6 M/s = k[0.00125 M]x[0.0088 M]y Eqn 1Rate of reaction for run 2= 1.58 x10-6 M/sRate law for Run 2 : 1.58 x10-6 M/s = k[0.0025 M]x[0.0088 M]y Eqn 2Rate of reaction for run 3 = 1.99 x10-6 M/sRate law for Run 3 : 1.99 x10-6 M/s = k[0.00125 M]x[0.0176 M]y Eqn 3 ---### Laboratory Report: Reaction Kinetics#### Mass of potassium iodide used: 0.12 g#### Mass of sodium thiosulfate pentahydrate used: 0.115 g#### Volume of 30% hydrogen peroxide: 2 mL#### Part A: Rate Law- **Temperature:** Not specified in text#### Experimental Runs:| | Run #1 | Run #2 | Run #3 ||----------------------|-----------------|-----------------|----------------|| **Time until permanent blue color appears** | | | || **Rate of reaction** | 1.08 × 10^-5 M/s | 1.58 × 10^-6 M/s | 1.99 × 10^-6 M/s || **Rate law** | | | || **Rate constant** | | | || **Temperature of solution** | | | | #### Handwritten Calculations and Notes:- Calculation of hydrogen peroxide volume: \[ \text{3 = V}_1 (V_1 + V_2) \times 30 \] \[ \text{3 = V}_1 (20 \times 30) \] \[ \text{V}_1 = (3 \times 20) / 30 = 2 \text{mL} \]- Calculation of molar amounts: \[ 0.025 \text{ mol/L} \times (50 \text{mL/L}) / (100\text{mL}) \] \[ = 0.025 \text{ mol/L} \times 0.050 \text{L} \] \[ = 0.00125 \text{ mol} \] \[ 0.00125 \text{ mol} \times 166.9 \frac{\text{g}}{\text{mol}} = 0.2\text{g} \](Note: Some calculations above might need clarification from the context provided in the lab manual or experimental details).---This transcription and explanation should provide a comprehensive overview of the experimental setup and findings for an educational website. Ensure all complex calculations are understood by cross-referencing them with the respective experiment guidelines and chemical principles ### Reaction Rate Experiment#### Components and Measurements:| Components | Run #1 | Run #2 | Run #3 ||--------------------------|---------------|---------------|---------------|| 0.36 M sulfuric acid | 35 mL | 35 mL | 35 mL || Deionized water | 48 mL | 43 mL | 47 mL || 0.025 M potassium iodide | 5 mL | 10 mL | 5 mL || 0.0025 M sodium thiosulfate | 10 mL | 10 mL | 10 mL || Starch solution | 1 mL | 1 mL | 1 mL |#### Procedure:1. **Mixing the Components**: - For Run #1, add the components in the order listed and mix the contents of the flask thoroughly before proceeding to steps 3-5.2. **Addition of Hydrogen Peroxide**: - Pipette 1.0 mL of 3% hydrogen peroxide into the flask and note the time of addition (3% hydrogen peroxide is equivalent to 0.88 M hydrogen peroxide).3. **Observation**: - Swirl the flask continuously and record, to the nearest second, how long it takes for a permanent blue-black color to appear. This time is the duration required for all the thiosulfate to react.4. **Measurement**: - Measure the temperature of the solution.5. **Repeat the Procedure**: - Repeat steps 3 - 5 for Run #2.6. **Hydrogen Peroxide in Run #3**: - Add 2.0 mL of 3% hydrogen peroxide and note the time of addition.7. **Observation and Timing**: - Swirl the flask continuously and record, to the nearest second, how long it takes for a permanent blue-black color to appear. This is the reaction time required for all the thiosulfate to react.#### Part B: Temperature Effect1. **Reaction at Different Temperatures**: - Repeat the reaction using the same amounts of reactants as for Run #3, but at different temperatures. - Use an ice bath to achieve a temperature of 5-10°C

The avbove reaction is done to determine the rate constant of decomposition of H2O2 by acidified KI…

Answered: Calculate the value of the rate…

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...