Determine the value of k (without units) for the reaction: C¿H¾B[2 + 3KI → C2H4 + 2KBr +Kl3, given the initial rate data below? [C;H&Brz], M [KI], M A[K!3]/At (M min"') 0.500 1.80 0.269 0.500 7.20 1.08 1.50 1.80 0.807 Select one: O a. 0.299 O b. 0.538 O c. 0.149 O d. 0.0830
Determine the value of k (without units) for the reaction: C¿H¾B[2 + 3KI → C2H4 + 2KBr +Kl3, given the initial rate data below? [C;H&Brz], M [KI], M A[K!3]/At (M min"') 0.500 1.80 0.269 0.500 7.20 1.08 1.50 1.80 0.807 Select one: O a. 0.299 O b. 0.538 O c. 0.149 O d. 0.0830
Chemistry
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Chapter1: Chemical Foundations
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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![### Reaction Rate Determination
#### Problem Statement
Determine the value of \( k \) (without units) for the reaction:
\[ \text{C}_2\text{H}_4\text{Br}_2 + 3\text{KI} \rightarrow \text{C}_2\text{H}_4 + 2\text{KBr} + \text{KI}_3 \]
given the initial rate data below?
#### Data Table:
| [C2H4Br2], M | [KI], M | Δ[KI3]/Δt (M min⁻¹) |
|--------------|---------|----------------------|
| 0.500 | 1.80 | 0.269 |
| 0.500 | 7.20 | 1.08 |
| 1.50 | 1.80 | 0.807 |
#### Multiple-Choice Options:
Select one:
- a. 0.299
- b. 0.538
- c. 0.149
- d. 0.0830
#### Diagrams
No graphs or diagrams are provided in the given question.
---
To solve for the rate constant \( k \), you can use the rate law and the data points provided. The rate law for this reaction can be written in the form:
\[ \text{rate} = k [\text{C}_2\text{H}_4\text{Br}_2]^m [\text{KI}]^n \]
By analyzing the changes in the concentration of reactants and their effect on the rate, the constants \( m \) and \( n \) and finally \( k \) can be determined.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F4c1ac660-1734-4e58-bb08-c8b54c6e23fd%2F14d4e962-c0e0-4030-91e3-b432535210e8%2Fh7gh8wf_processed.png&w=3840&q=75)
Transcribed Image Text:### Reaction Rate Determination
#### Problem Statement
Determine the value of \( k \) (without units) for the reaction:
\[ \text{C}_2\text{H}_4\text{Br}_2 + 3\text{KI} \rightarrow \text{C}_2\text{H}_4 + 2\text{KBr} + \text{KI}_3 \]
given the initial rate data below?
#### Data Table:
| [C2H4Br2], M | [KI], M | Δ[KI3]/Δt (M min⁻¹) |
|--------------|---------|----------------------|
| 0.500 | 1.80 | 0.269 |
| 0.500 | 7.20 | 1.08 |
| 1.50 | 1.80 | 0.807 |
#### Multiple-Choice Options:
Select one:
- a. 0.299
- b. 0.538
- c. 0.149
- d. 0.0830
#### Diagrams
No graphs or diagrams are provided in the given question.
---
To solve for the rate constant \( k \), you can use the rate law and the data points provided. The rate law for this reaction can be written in the form:
\[ \text{rate} = k [\text{C}_2\text{H}_4\text{Br}_2]^m [\text{KI}]^n \]
By analyzing the changes in the concentration of reactants and their effect on the rate, the constants \( m \) and \( n \) and finally \( k \) can be determined.
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