**Determine the Activation Energy for the Redox Reaction****Reaction:** \[ Q^{2+} + 2 \, R^{3+} \rightarrow Q^{4+} + 2 \, R^{2+} \]**Data Table**| Rate Constant (M⁻¹s⁻¹) | Temperature (K) ||------------------------|-----------------|| \(3.12 \times 10^3\) | 275 || \(2.70 \times 10^4\) | 300 |**Instructions:**To calculate the activation energy for the given redox reaction, you need to use 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 universal gas constant (8.314 J/mol·K),- \( T \) is the temperature in Kelvin.**Diagram Explanation:**No graphs or diagrams are present in the image. However, there is a numeric keypad on the right side, suggesting computational input for solving equations related to the reaction's activation energy.**Calculation:**You may compute the activation energy by rearranging the Arrhenius equation into its linear form and using the data provided in the table. Apply the natural logarithm to both sides and plot \(\ln k\) vs \(1/T\), or calculate directly if needed.

Name: **Determine the Activation Energy for the Redox Reaction****Reaction:
Uploaded: 2022-11-30T19:17:17.000Z
Channel: Bartleby
Description: **Determine the Activation Energy for the Redox Reaction****Reaction:** \[ Q^{2+} + 2 \, R^{3+} \rightarrow Q^{4+} + 2 \, R^{2+} \]**Data Table**| Rate Constant (M⁻¹s⁻¹) | Temperature (K) ||------------------------|-----------------|| \(3.12 \times

The rate constant of a reaction depends on the temperature of the reaction. The minimum amount of energy is needed by the reactants to take part in the reaction is called threshold energy. Activation energy is the amount of energy needed by the reactants molecule to reach that threshold energy level. The relation of rate constant with the temperature is shown below-log10k2k1=Ea2.303R1T1-1T2log102.70×1043.12×103=Ea2.303×8.3141275-1300log108.65=Ea2.303×8.314×2582500Ea=0.94×2.303×8.314×825002559394.43JEa=59394.43J=59.39KJFor one mole, divide this activation energy by Avogadro's number,Ea=59.39KJ6.022×1023=9.86×10-23KJ/mole