# Using the Arrhenius Equation to Calculate k at One Temperature**Topic:** Kinetics and EquilibriumThe rate constant of a certain reaction is known to obey the Arrhenius equation and has an activation energy $ E_a = 57.0 \, \text{kJ/mol} $. If the rate constant of this reaction is $ 0.15 \, \text{M}^{-1} \, \text{s}^{-1} $ at $ 20.0^\circ \text{C} $, what will the rate constant be at $-82.0^\circ \text{C}$?**Instructions:** Round your answer to 2 significant digits.### Formula\[ k = A e^{\frac{-E_a}{RT}} \]### Variables- $ k $: Rate constant- $ E_a $: Activation energy- $ R $: Universal gas constant- $ T $: Temperature in Kelvin### Input Boxes- **k:** [ ]- **M$^-1$:** [$\square$]- **s$^-1$:** [$\square$]**Buttons:**- Explanation: [ ]- Check: [ ]**Note:** Ensure all calculations consider the conversion of temperature from Celsius to Kelvin.This exercise aims to apply the Arrhenius equation to determine the change in the rate constant with temperature, underlining the effect of temperature on reaction rates.

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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-57.0 kJ/mol. If the rate constant of this -1 reaction is 0.15 Ms at 2.0 °C, what will the rate constant be at -82.0 °C? Round your answer to 2 significant digits. -1 k=M²¹-5 X $

The rate constant of a certain reaction is known to obey the Arrhenius equation, and to have an activation energy E-57.0 kJ/mol. If the rate constant of this -1 reaction is 0.15 Ms at 2.0 °C, what will the rate constant be at -82.0 °C? Round your answer to 2 significant digits. -1 k=M²¹-5 X $

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...

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