### Reaction Rate Constants and Activation EnergyThe rate constant \( k \) for a certain reaction is measured at two different temperatures and given in the following table:| Temperature (°C) | \( k \) (1/s) ||-------------------------|--------:|| 401.0 °C | 5.2 × 10\(^9\) || 270.0 °C | 2.7 × 10\(^9\) |Assuming the rate constant follows the Arrhenius equation, calculate the activation energy \( E_a \) for this reaction. Round your answer to 2 significant digits.The Arrhenius equation is given as:\[ E_a = \boxed{ \ \ \ \ \ \ \ \ } \text{kJ/mol}\]Note: The text accompanying the activation energy equation is missing, but typically, the relationship used is:\[ E_a = \frac{R \cdot (T_1 \cdot T_2)}{T_2 - T_1} \cdot \ln \left( \frac{k_2}{k_1} \right) \]where:- \( k_1 \) and \( k_2 \) are the rate constants at temperatures \( T_1 \) and \( T_2 \) respectively,- \( R \) is the gas constant, often taken as \( 8.314 \) J/(mol·K),- \( T_1 \) and \( T_2 \) are absolute temperatures in Kelvin.To convert temperatures from Celsius to Kelvin, add 273.15 to the value in Celsius:\[ T_{Kelvin} = T_{Celsius} + 273.15 \]

Name: ### Reaction Rate Constants and Activation EnergyThe rate constant \(
Uploaded: 2022-11-30T19:17:17.000Z
Channel: Bartleby
Description: ### Reaction Rate Constants and Activation EnergyThe rate constant \( k \) for a certain reaction is measured at two different temperatures and given in the following table:| Temperature (°C) | \( k \) (1/s) ||-------------------------|--------:|| 4