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The rate constant of a certain reaction is known to obey the Arrhenius equation, and to have an activation energy E-5.0 kJ/mol. If the rate constant of this reaction is 3.3 x 10 Ms at 275.0 °C, what will the rate constant be at 354.0 °C? Round your answer to 2 significant digits. K=OM²¹²¹

The rate constant of a certain reaction is known to obey the Arrhenius equation, and to have an activation energy E-5.0 kJ/mol. If the rate constant of this reaction is 3.3 x 10 Ms at 275.0 °C, what will the rate constant be at 354.0 °C? Round your answer to 2 significant digits. K=OM²¹²¹

Chemistry
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
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The image displays a problem related to chemical kinetics and the Arrhenius equation. It reads: **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 \( E_a = 5.0 \, \text{kJ/mol} \). If the rate constant of this reaction is \( 3.3 \times 10^{-7} \, \text{M}^{-1} \, \text{s}^{-1} \) at \( 275.0^\circ \text{C} \), what will the rate constant be at \( 354.0^\circ \text{C} \)? Round your answer to 2 significant digits. There is an input box for the user to enter the calculated rate constant in \( \text{M}^{-1} \, \text{s}^{-1} \). Buttons available: - Explanation - Check Below the problem is the interface of a MacBook Pro keyboard and desktop, with some application icons visible but irrelevant to the educational content. No graphs or diagrams are present in the image.
Transcribed Image Text:The image displays a problem related to chemical kinetics and the Arrhenius equation. It reads: **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 \( E_a = 5.0 \, \text{kJ/mol} \). If the rate constant of this reaction is \( 3.3 \times 10^{-7} \, \text{M}^{-1} \, \text{s}^{-1} \) at \( 275.0^\circ \text{C} \), what will the rate constant be at \( 354.0^\circ \text{C} \)? Round your answer to 2 significant digits. There is an input box for the user to enter the calculated rate constant in \( \text{M}^{-1} \, \text{s}^{-1} \). Buttons available: - Explanation - Check Below the problem is the interface of a MacBook Pro keyboard and desktop, with some application icons visible but irrelevant to the educational content. No graphs or diagrams are present in the image.
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To calculate the value of rate constant we would use Arrhenius equation. 

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