Chemistry
Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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Question
**Question 2: Determining Activation Energy** At 32.0°C, the rate constant of a reaction is 0.0550 s⁻¹. Given that the frequency factor is 1.20 x 10¹³ s⁻¹, calculate the activation energy. --- To solve this problem, you can use the Arrhenius equation: \[ k = A e^{-E_a/(RT)} \] Where: - \( k \) is the rate constant, - \( A \) is the frequency factor, - \( E_a \) is the activation energy, - \( R \) is the universal gas constant (8.314 J/mol·K), - \( T \) is the temperature in Kelvin. **Steps to solve:** 1. Convert the given temperature from Celsius to Kelvin by adding 273.15. 2. Rearrange the Arrhenius equation to solve for the activation energy \( E_a \). 3. Substitute the given values and constants into the equation. 4. Solve for \( E_a \). Note: Pay careful attention to units throughout the calculation to ensure accuracy.
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Transcribed Image Text:**Question 2: Determining Activation Energy** At 32.0°C, the rate constant of a reaction is 0.0550 s⁻¹. Given that the frequency factor is 1.20 x 10¹³ s⁻¹, calculate the activation energy. --- To solve this problem, you can use the Arrhenius equation: \[ k = A e^{-E_a/(RT)} \] Where: - \( k \) is the rate constant, - \( A \) is the frequency factor, - \( E_a \) is the activation energy, - \( R \) is the universal gas constant (8.314 J/mol·K), - \( T \) is the temperature in Kelvin. **Steps to solve:** 1. Convert the given temperature from Celsius to Kelvin by adding 273.15. 2. Rearrange the Arrhenius equation to solve for the activation energy \( E_a \). 3. Substitute the given values and constants into the equation. 4. Solve for \( E_a \). Note: Pay careful attention to units throughout the calculation to ensure accuracy.
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