7. Substances P and Q react together to form products and the overall order of the reaction is three. Which of the following rate equations could not be correct and why? A rate = k [P]2 [Q] D rate = k [P][Q]³ E rate = K[P][Q]²[H*]° B rate= k [P] [Q]³ C rate = k [P] [Q]² 2.1, 2.2 L3 8. The reaction between three reactants A, B and C was studied. The initial rates of reaction at different concentrations of the three reactants were measured and are given in the following table: [A]/mol dm3 [B]/mol dm3 [C]/mol dm-3 1.0 3.0 3.0 1.0 experiment 1 2 a) b) c) 3 4 1.0 1.0 2.0 2.0 1.0 1.0 1.0 2.0 Deduce the partial orders of reaction with respect to A, B and C. Calculate the value of the rate constant, giving its units. Write the rate equation. Initial rate/mol dm³ s-1 2.3x10-3 6.9×10-3 1.4×10-² 4.6×10-3 21.2.2L3
7. Substances P and Q react together to form products and the overall order of the reaction is three. Which of the following rate equations could not be correct and why? A rate = k [P]2 [Q] D rate = k [P][Q]³ E rate = K[P][Q]²[H*]° B rate= k [P] [Q]³ C rate = k [P] [Q]² 2.1, 2.2 L3 8. The reaction between three reactants A, B and C was studied. The initial rates of reaction at different concentrations of the three reactants were measured and are given in the following table: [A]/mol dm3 [B]/mol dm3 [C]/mol dm-3 1.0 3.0 3.0 1.0 experiment 1 2 a) b) c) 3 4 1.0 1.0 2.0 2.0 1.0 1.0 1.0 2.0 Deduce the partial orders of reaction with respect to A, B and C. Calculate the value of the rate constant, giving its units. Write the rate equation. Initial rate/mol dm³ s-1 2.3x10-3 6.9×10-3 1.4×10-² 4.6×10-3 21.2.2L3
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
Chapter12: Chemical Kinetics
Section: Chapter Questions
Problem 121CP: Consider the hypothetical reaction A+B+2C2D+3E In a study of this reaction three experiments were...
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![### Chemical Kinetics: Rate Equations and Reaction Orders
**7. Substances P and Q react together to form products and the overall order of the reaction is three. Which of the following rate equations could not be correct and why?**
- **A**: rate = k \[P\]^2 \[Q\]
- **B**: rate = k \[P\]^0 \[Q\]^3
- **C**: rate = k \[P\] \[Q\]^2
- **D**: rate = k \[P\] \[Q\]^3
- **E**: rate = k \[P\] \[Q\]^2 \[H\]^0
**8. The reaction between three reactants A, B, and C was studied. The initial rates of reaction at different concentrations of the three reactants were measured and are given in the following table:**
| experiment | \[A\] / mol dm<sup>-3</sup> | \[B\] / mol dm<sup>-3</sup> | \[C\] / mol dm<sup>-3</sup> | Initial rate / mol dm<sup>-3</sup> s<sup>-1</sup> |
|--|--|--|--|--|
| 1 | 1.0 | 1.0 | 1.0 | 2.3 × 10<sup>-3</sup> |
| 2 | 1.0 | 3.0 | 1.0 | 6.9 × 10<sup>-3</sup> |
| 3 | 2.0 | 3.0 | 1.0 | 1.4 × 10<sup>-2</sup> |
| 4 | 2.0 | 1.0 | 2.0 | 4.6 × 10<sup>-3</sup> |
#### a) Deduce the partial orders of reaction with respect to A, B, and C.
#### b) Calculate the value of the rate constant, giving its units.
#### c) Write the rate equation.
**Graph/Diagram Explanation:**
The table provided in question 8 lists the concentrations of reactants A, B, and C in different experiments along with the initial rates of reaction. This data can](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fb5386f0c-0c7d-4f0c-9c77-b0195c82b8c2%2F5e10053b-b6ba-4e82-a47b-af4f7c8a5ce7%2Fqfspk0m_processed.jpeg&w=3840&q=75)
Transcribed Image Text:### Chemical Kinetics: Rate Equations and Reaction Orders
**7. Substances P and Q react together to form products and the overall order of the reaction is three. Which of the following rate equations could not be correct and why?**
- **A**: rate = k \[P\]^2 \[Q\]
- **B**: rate = k \[P\]^0 \[Q\]^3
- **C**: rate = k \[P\] \[Q\]^2
- **D**: rate = k \[P\] \[Q\]^3
- **E**: rate = k \[P\] \[Q\]^2 \[H\]^0
**8. The reaction between three reactants A, B, and C was studied. The initial rates of reaction at different concentrations of the three reactants were measured and are given in the following table:**
| experiment | \[A\] / mol dm<sup>-3</sup> | \[B\] / mol dm<sup>-3</sup> | \[C\] / mol dm<sup>-3</sup> | Initial rate / mol dm<sup>-3</sup> s<sup>-1</sup> |
|--|--|--|--|--|
| 1 | 1.0 | 1.0 | 1.0 | 2.3 × 10<sup>-3</sup> |
| 2 | 1.0 | 3.0 | 1.0 | 6.9 × 10<sup>-3</sup> |
| 3 | 2.0 | 3.0 | 1.0 | 1.4 × 10<sup>-2</sup> |
| 4 | 2.0 | 1.0 | 2.0 | 4.6 × 10<sup>-3</sup> |
#### a) Deduce the partial orders of reaction with respect to A, B, and C.
#### b) Calculate the value of the rate constant, giving its units.
#### c) Write the rate equation.
**Graph/Diagram Explanation:**
The table provided in question 8 lists the concentrations of reactants A, B, and C in different experiments along with the initial rates of reaction. This data can
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