The reaction: 2 clO2 (aq) → ClO3- (ag) + C1O2¯ (ag) + H2O studied with the following experimental results: Molarity (Na) STOCK (0.09 +2 OH- + CIO2 (ag) + H20 0, was (aq) Final Be Conce Vol (ml) Trial # Rate/M-sec [CIO2/M 0.060 [OH/M 0.030 1 0.0248 0.020 0.030 0.00276 3 0.020 0.090 0.00828 The general expression for the rate law is Rate = k[CIO2]™[OH¯]". Derive the reaction orders, m and n, for the reaction. Show all work. 1. %3D nldn and study the Go to this rinod information provided in the Table(s) above the vialts) smmarized Chemical Bleach Bleach Conc (M) 0.090 Volume (mL) 0.50 0.50 0.180 Yellow Dye 3.40E-05 10.0 Note: there is no "dio"-You s index finger pointing to the bleach be this 2. Use any one(1) of the three trials shown in part 1 to calculate the rate constant k. Show all work. Dil. Bleach tions of Dye, Conc. mixing Blcach the video reactants
The reaction: 2 clO2 (aq) → ClO3- (ag) + C1O2¯ (ag) + H2O studied with the following experimental results: Molarity (Na) STOCK (0.09 +2 OH- + CIO2 (ag) + H20 0, was (aq) Final Be Conce Vol (ml) Trial # Rate/M-sec [CIO2/M 0.060 [OH/M 0.030 1 0.0248 0.020 0.030 0.00276 3 0.020 0.090 0.00828 The general expression for the rate law is Rate = k[CIO2]™[OH¯]". Derive the reaction orders, m and n, for the reaction. Show all work. 1. %3D nldn and study the Go to this rinod information provided in the Table(s) above the vialts) smmarized Chemical Bleach Bleach Conc (M) 0.090 Volume (mL) 0.50 0.50 0.180 Yellow Dye 3.40E-05 10.0 Note: there is no "dio"-You s index finger pointing to the bleach be this 2. Use any one(1) of the three trials shown in part 1 to calculate the rate constant k. Show all work. Dil. Bleach tions of Dye, Conc. mixing Blcach the video reactants
Chemistry
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...
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Please answer the questions on the pictures provided
![**Educational Resource: Reaction Rate Analysis**
The chemical reaction under study is:
\[ 2 \text{ClO}_2 (aq) + 2 \text{OH}^- (aq) \rightarrow \text{ClO}_3^- (aq) + \text{ClO}_2^- (aq) + \text{H}_2O (l) \]
The following experimental results were obtained:
| **Trial #** | **[ClO₂]/M** | **[OH⁻]/M** | **Rate/M·sec⁻¹** |
|-------------|--------------|-------------|----------------|
| 1 | 0.060 | 0.030 | 0.0248 |
| 2 | 0.020 | 0.030 | 0.00276 |
| 3 | 0.020 | 0.090 | 0.00828 |
1. **Rate Law Expression Derivation**:
The general expression for the rate law is determined as:
\[
\text{Rate} = k[\text{ClO}_2]^m[\text{OH}^-]^n
\]
Derive the reaction orders, \( m \) and \( n \), by analyzing the experimental data. Show all your work.
2. **Calculation of the Rate Constant (k)**:
Use any one of the three trials provided to calculate the rate constant \( k \). Ensure to show all your work.
3. **Stock Solution Volume Calculation**:
Calculate the volumes needed to make 10 mL of diluted NaOH solutions as per Table 2 (refer to the next page for Table 2). Follow Part I of the procedure and the provided flow chart. An example calculation should be demonstrated in the space below.
For detailed instructions and procedural steps, refer to the accompanying documentation and visual aids. Each calculation aims to enhance understanding of the chemical kinetics associated with this reaction.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F523b9775-526c-4840-92de-ec581e259b38%2F26af96f7-cfc2-4187-ad33-6727cdc106e8%2Fj84glu8_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Educational Resource: Reaction Rate Analysis**
The chemical reaction under study is:
\[ 2 \text{ClO}_2 (aq) + 2 \text{OH}^- (aq) \rightarrow \text{ClO}_3^- (aq) + \text{ClO}_2^- (aq) + \text{H}_2O (l) \]
The following experimental results were obtained:
| **Trial #** | **[ClO₂]/M** | **[OH⁻]/M** | **Rate/M·sec⁻¹** |
|-------------|--------------|-------------|----------------|
| 1 | 0.060 | 0.030 | 0.0248 |
| 2 | 0.020 | 0.030 | 0.00276 |
| 3 | 0.020 | 0.090 | 0.00828 |
1. **Rate Law Expression Derivation**:
The general expression for the rate law is determined as:
\[
\text{Rate} = k[\text{ClO}_2]^m[\text{OH}^-]^n
\]
Derive the reaction orders, \( m \) and \( n \), by analyzing the experimental data. Show all your work.
2. **Calculation of the Rate Constant (k)**:
Use any one of the three trials provided to calculate the rate constant \( k \). Ensure to show all your work.
3. **Stock Solution Volume Calculation**:
Calculate the volumes needed to make 10 mL of diluted NaOH solutions as per Table 2 (refer to the next page for Table 2). Follow Part I of the procedure and the provided flow chart. An example calculation should be demonstrated in the space below.
For detailed instructions and procedural steps, refer to the accompanying documentation and visual aids. Each calculation aims to enhance understanding of the chemical kinetics associated with this reaction.
 and study the information provided in the Table(s) about the vial(s) summarized here:
| Chemical | Conc (M) | Volume (mL) |
|-------------|-----------|-------------|
| Bleach | 0.090 | 0.50 |
| Bleach | 0.180 | 0.50 |
| Yellow Dye | 3.40E-05 | 10.0 |
*Note: there is no “audio” - You must look at his index finger pointing to the bleach being used in each trial.*
**NOTE:** Do the following calculations using this data in the Table above:
Calculate the **initial** concentrations of Dye, Conc. Bleach, and Dil. Bleach in each reactor vial **immediately** after mixing the two reactants in the video.
*HINT: pretend/assume the yellow dye is 100% pure solvent used as a diluent.*
---
*(Please perform the calculations and fill in the missing data to complete the exercise.)*](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F523b9775-526c-4840-92de-ec581e259b38%2F26af96f7-cfc2-4187-ad33-6727cdc106e8%2Fevmbs0g_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Transcription for Educational Website**
---
**Chem 112 Lab: Kinetics of Crystal Violet Bleaching**
**4.** Next, look at the actual reaction dilution ratio when CV and NaOH is mixed to commence bleaching. Calculate the final NaOH concentration in the reaction beaker just before an aliquot is placed in the cuvette for analysis. Add values into the last column below. One sample calculation in space here:
**TABLE 2:**
| Molarity (NaOH) STOCK (0.050 M) | Vol (mL) Stock Solution | Vol (mL) Water | Final Reaction OH⁻ Concentration (NaOH) |
|---------------------------------|-------------------------|---------------|-----------------------------------------|
| 0.050 | ~50 | 0.0 | 0.0 M |
| 0.040 | | | |
| 0.030 | | | |
| 0.020 | | | |
| 0.010 | | | |
**5.** Go to this link: [YouTube Video](https://www.youtube.com/watch?v=40Y_oldmNVk&t=15s) and study the information provided in the Table(s) about the vial(s) summarized here:
| Chemical | Conc (M) | Volume (mL) |
|-------------|-----------|-------------|
| Bleach | 0.090 | 0.50 |
| Bleach | 0.180 | 0.50 |
| Yellow Dye | 3.40E-05 | 10.0 |
*Note: there is no “audio” - You must look at his index finger pointing to the bleach being used in each trial.*
**NOTE:** Do the following calculations using this data in the Table above:
Calculate the **initial** concentrations of Dye, Conc. Bleach, and Dil. Bleach in each reactor vial **immediately** after mixing the two reactants in the video.
*HINT: pretend/assume the yellow dye is 100% pure solvent used as a diluent.*
---
*(Please perform the calculations and fill in the missing data to complete the exercise.)*
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