O KINETICS AND EQUILIBRIUM Using the Arrhenius equation to calculate k at one temperature... The rate constant of a certain reaction is known to obey the Arrhenius equation, and to have an activation energy E-29.0 kJ/mol. If the rate constant of this -1 reaction is 2.8 x 10³ Ms at 320.0 °C, what will the rate constant be at 222.0 °C? Round your answer to 2 significant digits. k= X ? olo
O KINETICS AND EQUILIBRIUM Using the Arrhenius equation to calculate k at one temperature... The rate constant of a certain reaction is known to obey the Arrhenius equation, and to have an activation energy E-29.0 kJ/mol. If the rate constant of this -1 reaction is 2.8 x 10³ Ms at 320.0 °C, what will the rate constant be at 222.0 °C? Round your answer to 2 significant digits. k= X ? olo
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...
Related questions
Question
![The image displays a problem related to chemical kinetics, specifically involving the Arrhenius equation. This is a common task on an educational platform, likely for homework or practice.
### Problem Statement:
"The rate constant of a certain reaction is known to obey the Arrhenius equation, and to have an activation energy \( E_{\text{a}} = 29.0 \, \text{kJ/mol} \). If the rate constant of this reaction is \( 2.8 \times 10^{5} \, \text{M}^{-1}\text{s}^{-1} \) at 320.0 °C, what will the rate constant be at 222.0 °C?
Round your answer to 2 significant digits."
### Interactive Features:
- **Input Box**: A field where users can input their calculated rate constant.
- **Units**: The unit of the rate constant is specified as \(\text{M}^{-1}\text{s}^{-1}\).
- **Buttons**:
- **Check**: After entering a value, users can click this button to verify if their answer is correct.
- **Explanation**: Likely provides a detailed solution or hints for understanding the process to reach the correct answer.
### Additional Context:
- **Arrhenius Equation**: A formula used to calculate the rate constant of a reaction at different temperatures, typically expressed as:
\[
k = A e^{-\frac{E_{\text{a}}}{RT}}
\]
where \( k \) is the rate constant, \( A \) is the pre-exponential factor, \( E_{\text{a}} \) is the activation energy, \( R \) is the gas constant, and \( T \) is the temperature in Kelvin.
This problem requires understanding of kinetic principles and mathematical calculations using the Arrhenius equation to determine the effect of temperature change on the rate constant.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F1ac9d9fd-0ce6-4ad9-ac74-440cab402247%2Fc67d8ad7-c058-42b2-8d2d-d3d6d8009356%2Fve6p0au_processed.jpeg&w=3840&q=75)
Transcribed Image Text:The image displays a problem related to chemical kinetics, specifically involving the Arrhenius equation. This is a common task on an educational platform, likely for homework or practice.
### Problem Statement:
"The rate constant of a certain reaction is known to obey the Arrhenius equation, and to have an activation energy \( E_{\text{a}} = 29.0 \, \text{kJ/mol} \). If the rate constant of this reaction is \( 2.8 \times 10^{5} \, \text{M}^{-1}\text{s}^{-1} \) at 320.0 °C, what will the rate constant be at 222.0 °C?
Round your answer to 2 significant digits."
### Interactive Features:
- **Input Box**: A field where users can input their calculated rate constant.
- **Units**: The unit of the rate constant is specified as \(\text{M}^{-1}\text{s}^{-1}\).
- **Buttons**:
- **Check**: After entering a value, users can click this button to verify if their answer is correct.
- **Explanation**: Likely provides a detailed solution or hints for understanding the process to reach the correct answer.
### Additional Context:
- **Arrhenius Equation**: A formula used to calculate the rate constant of a reaction at different temperatures, typically expressed as:
\[
k = A e^{-\frac{E_{\text{a}}}{RT}}
\]
where \( k \) is the rate constant, \( A \) is the pre-exponential factor, \( E_{\text{a}} \) is the activation energy, \( R \) is the gas constant, and \( T \) is the temperature in Kelvin.
This problem requires understanding of kinetic principles and mathematical calculations using the Arrhenius equation to determine the effect of temperature change on the rate constant.
Expert Solution
Step 1
Given,
Activation energy (Ea) = 29.0 kJ/mol = 29.0 × 1000 J/mol = 29000 J/mol
Rate constant (k):
k1 = 2.8 × 105 M-1.s-1
k2 = ?
Temperature (T):
T1 = 320.0°C = (320.0 + 273.15)K = 593.15 K
T2 = 222.0°C = (222.0 + 273.15)K = 495.15 K
Note: universal gas constant (R) = 8.314 J/mol.K
Step by step
Solved in 3 steps with 1 images
Knowledge Booster
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.Recommended textbooks for you
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
Organic Chemistry
Chemistry
ISBN:
9780078021558
Author:
Janice Gorzynski Smith Dr.
Publisher:
McGraw-Hill Education
Chemistry: Principles and Reactions
Chemistry
ISBN:
9781305079373
Author:
William L. Masterton, Cecile N. Hurley
Publisher:
Cengage Learning
Elementary Principles of Chemical Processes, Bind…
Chemistry
ISBN:
9781118431221
Author:
Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:
WILEY