**Chemical Reaction and Activation Energy Calculation**The given reaction is:\[ \text{C}_4\text{H}_8\text{(g)} \rightarrow 2 \, \text{C}_2\text{H}_4\text{(g)} \]This reaction has an activation energy of 262 kJ/mol. At a temperature of 600.0 K, the rate constant (\(k\)) is \(6.1 \times 10^{-8} \, \text{s}^{-1}\). We are tasked with finding the value of the rate constant at 745.0 K.**Formula to Use:**The relation between the rate constants at two different temperatures can be determined using the Arrhenius equation:\[ k = A \, e^{-\frac{E_a}{RT}} \]Where:- \(k\) is the rate constant,- \(A\) is the pre-exponential factor,- \(E_a\) is the activation energy,- \(R\) is the gas constant (8.314 J/mol·K),- \(T\) is the temperature in Kelvin.**Comparison of Rate Constants:**To find the rate constant at the new temperature (745.0 K), the Arrhenius equation can be rearranged to the following form for practical use:\[ \ln \left( \frac{k_2}{k_1} \right) = -\frac{E_a}{R} \left( \frac{1}{T_2} - \frac{1}{T_1} \right) \]Where:- \(k_1\) and \(k_2\) are the rate constants at temperatures \(T_1\) and \(T_2\) respectively,- \(T_1\) is 600.0 K,- \(T_2\) is 745.0 K.**Calculate \(k\):**Insert the given values to solve for \(k\) at 745.0 K in the provided box.\[ k = \, \square \, \text{s}^{-1} \]

Two point Arrhenius equation is given by, Where, Ea is the…

Answered: The reaction C,H, (g) → 2C,H,(g) has an…

The reaction C,H, (g) → 2C,H,(g) has an activation energy of 262 kJ/mol. At 600.0 K, the rate constant, k, is 6.1 × 10-8 s-1. What is the value of the rate constant at 745.0 K? k =

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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