**Reaction Rate Constant and Activation Energy Calculation**The rate constant \( k \) for a certain reaction is measured at two different temperatures as shown in the table below:| Temperature (°C) | \( k \) (s\(^{-1}\)) ||------------------|----------------------|| 264.0 °C | \( 4.4 \times 10^8 \)|| 163.0 °C | \( 1.9 \times 10^8 \)|### Problem StatementAssuming the rate constant obeys the Arrhenius equation, calculate the activation energy \( E_a \) for this reaction.Round your answer to 2 significant digits.### Formula for Activation Energy\[ E_a = \boxed{ \quad } \text{ kJ/mol} \]### Instructions1. Utilize the Arrhenius equation:\[ k = A \exp\left(\frac{-E_a}{RT}\right) \]Where: - \( k \) = rate constant, - \( A \) = pre-exponential factor, - \( E_a \) = activation energy, - \( R \) = gas constant (\(8.314 \text{ J·mol}^{-1}\text{·K}^{-1}\)), - \( T \) = temperature in Kelvin.2. Convert temperatures from Celsius to Kelvin: - \( T_1 = 264.0 °C + 273.15 = 537.15 \text{ K} \) - \( T_2 = 163.0 °C + 273.15 = 436.15 \text{ K} \)3. Apply the natural logarithm form of the Arrhenius equation to find \( E_a \):\[ \ln\left(\frac{k_1}{k_2}\right) = \frac{E_a}{R} \left(\frac{1}{T_2} - \frac{1}{T_1}\right) \]By solving this equation, you can determine the activation energy \( E_a \).

Name: **Reaction Rate Constant and Activation Energy Calculation**The rate
Uploaded: 2022-11-30T19:17:17.000Z
Channel: Bartleby
Description: **Reaction Rate Constant and Activation Energy Calculation**The rate constant \( k \) for a certain reaction is measured at two different temperatures as shown in the table below:| Temperature (°C) | \( k \) (s\(^{-1}\)) ||------------------|-------