### Calculating the Activation Energy Using the Arrhenius Equation**Problem Statement:**The rate constant \( k \) for a certain reaction is measured at two different temperatures:| Temperature (°C) | \( k \) ||------------------|----------------------------------|| 74.0 °C | \( 9.8 \times 10^{12} \) || 197.0 °C | \( 9.6 \times 10^{15} \) |**Objective:**Assuming the rate constant obeys the Arrhenius equation, calculate the activation energy \( E_a \) for this reaction.**Instructions:**1. Use the given temperatures and rate constants to calculate the activation energy.2. Round your answer to 2 significant digits.**Formula to Use:**The Arrhenius equation is given by:\[ k = A \cdot e^{-\frac{E_a}{RT}} \]Where:- \( k \) is the rate constant- \( A \) is the pre-exponential factor- \( E_a \) is the activation energy- \( R \) is the universal gas constant (8.314 J/(mol·K))- \( T \) is the temperature in KelvinTo solve for \( E_a \), we use the equation:\[ \ln\left(\frac{k_2}{k_1}\right) = \frac{E_a}{R} \left(\frac{1}{T_1} - \frac{1}{T_2}\right) \]**Graph Explanation:**No graphs are provided in this problem. Only tabulated data for temperatures and rate constants are given.**Calculation Panel:**The panel below allows you to enter your calculated value for \( E_a \) in kJ/mol.\[ E_a = \boxed{} \ \text{kJ/mol} \](Use the input box for calculations and rounding utilities.)Ensure to convert the activation energy from J/mol to kJ/mol by dividing by 1000. Finally, remember to round off to 2 significant digits.

Name: ### Calculating the Activation Energy Using the Arrhenius Equation**P
Uploaded: 2022-11-30T19:17:17.000Z
Channel: Bartleby
Description: ### Calculating the Activation Energy Using the Arrhenius Equation**Problem Statement:**The rate constant \( k \) for a certain reaction is measured at two different temperatures:| Temperature (°C) | \( k \) ||--------------