Questions. 1. The following data were collected at 20°C for the reaction of bromphenol blue (HBPB2) and hydroxide ions (OH) is shown below HBPB²- + OH + BPB3- + H2O The times required to consume a small but constant amount of HBPB2- at varying initial HBPB2- and OH- concentrations were measured and are recorded below. Determination [HBPB²-], M |[OH], M Time, s 1 7.22 x 10-6 1.00 75 7.22 x 10-6 0.25 290 3 3.63 x 10-6 1.00 152 Rate 2/Rate 1 =) = k[A]*[B]/k[A]*[B]° Calculate the rate constant for this reaction at room temperature.
Questions. 1. The following data were collected at 20°C for the reaction of bromphenol blue (HBPB2) and hydroxide ions (OH) is shown below HBPB²- + OH + BPB3- + H2O The times required to consume a small but constant amount of HBPB2- at varying initial HBPB2- and OH- concentrations were measured and are recorded below. Determination [HBPB²-], M |[OH], M Time, s 1 7.22 x 10-6 1.00 75 7.22 x 10-6 0.25 290 3 3.63 x 10-6 1.00 152 Rate 2/Rate 1 =) = k[A]*[B]/k[A]*[B]° Calculate the rate constant for this reaction at room temperature.
Chemistry
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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
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1. base on the data，what how do we find rate constant for this reaction at room temperature？
2. what cause the formation of the purple color ？？
![## Questions
1. **The following data were collected at 20ºC for the reaction of bromphenol blue (HBPB²⁻) and hydroxide ions (OH⁻) is shown below:**
\[
\text{HBPB}^{2-} + \text{OH}^{-} \leftrightarrow \text{BPB}^{3-} + \text{H}_2\text{O}
\]
**The times required to consume a small but constant amount of HBPB²⁻ at varying initial HBPB²⁻ and OH⁻ concentrations were measured and are recorded below:**
| Determination | \([\text{HBPB}^{2-}]\), M | \([\text{OH}^{-}]\), M | Time, s |
|:-------------:|:-------------------------:|:---------------------:|:-------:|
| 1 | 7.22 x 10⁻⁶ | 1.00 | 75 |
| 2 | 7.22 x 10⁻⁶ | 0.25 | 290 |
| 3 | 3.63 x 10⁻⁶ | 1.00 | 152 |
\[
\text{Rate 2/Rate 1} = \frac{k[\text{A}]^{x}[\text{B}]^{y}}{k[\text{A}]^{x}[\text{B}]^{y}}
\]
*Calculate the rate constant for this reaction at room temperature.*
2. **What causes the formation of the purple color that indicates that all of \( S_2O_3^{2-} \) has reacted?**
---
**Explanation of Graphs or Diagrams:**
The table represents the experimental data collected to study the reaction kinetics of the reaction between bromphenol blue (HBPB²⁻) and hydroxide ions (OH⁻). The columns represent different determinations with varying concentrations of the reactants and the recorded times at which a specific amount of HBPB²⁻ has been consumed during the reaction.
Instructions **for Calculating the Rate Constant:**
1. Use the data from the table to write down the rate equations for each of the determinations.
2.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Ff7e0b628-1887-4036-8cfa-486903c53c1e%2F74b00b8a-376c-46a9-863f-8ff51bfa3137%2F5e6pxfj_processed.jpeg&w=3840&q=75)
Transcribed Image Text:## Questions
1. **The following data were collected at 20ºC for the reaction of bromphenol blue (HBPB²⁻) and hydroxide ions (OH⁻) is shown below:**
\[
\text{HBPB}^{2-} + \text{OH}^{-} \leftrightarrow \text{BPB}^{3-} + \text{H}_2\text{O}
\]
**The times required to consume a small but constant amount of HBPB²⁻ at varying initial HBPB²⁻ and OH⁻ concentrations were measured and are recorded below:**
| Determination | \([\text{HBPB}^{2-}]\), M | \([\text{OH}^{-}]\), M | Time, s |
|:-------------:|:-------------------------:|:---------------------:|:-------:|
| 1 | 7.22 x 10⁻⁶ | 1.00 | 75 |
| 2 | 7.22 x 10⁻⁶ | 0.25 | 290 |
| 3 | 3.63 x 10⁻⁶ | 1.00 | 152 |
\[
\text{Rate 2/Rate 1} = \frac{k[\text{A}]^{x}[\text{B}]^{y}}{k[\text{A}]^{x}[\text{B}]^{y}}
\]
*Calculate the rate constant for this reaction at room temperature.*
2. **What causes the formation of the purple color that indicates that all of \( S_2O_3^{2-} \) has reacted?**
---
**Explanation of Graphs or Diagrams:**
The table represents the experimental data collected to study the reaction kinetics of the reaction between bromphenol blue (HBPB²⁻) and hydroxide ions (OH⁻). The columns represent different determinations with varying concentrations of the reactants and the recorded times at which a specific amount of HBPB²⁻ has been consumed during the reaction.
Instructions **for Calculating the Rate Constant:**
1. Use the data from the table to write down the rate equations for each of the determinations.
2.
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