Calculate the rate constant, k, for a reaction at 60.0 °C that has an activation energy of 77.7 kJ/mol and a frequency factor of 6.59 x 10" s-1. k =

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**Problem: Calculate the Rate Constant**

Calculate the rate constant, \( k \), for a reaction at 60.0 °C that has an activation energy of 77.7 kJ/mol and a frequency factor of \( 6.59 \times 10^{11} \, \text{s}^{-1} \).

**Solution:**

To calculate the rate constant \( k \), use the Arrhenius equation:
\[ k = A e^{-\frac{E_a}{RT}} \]

where:
- \( k \) is the rate constant,
- \( A \) is the frequency factor (\( 6.59 \times 10^{11} \, \text{s}^{-1} \)),
- \( E_a \) is the activation energy (77.7 kJ/mol),
- \( R \) is the gas constant (8.314 J/(mol·K)),
- \( T \) is the temperature in Kelvin (60.0 °C = 333.15 K).

Enter the calculated value of \( k \) in the provided box:

\[ k = \_\_\_\_\_\_\_\_\_\_ \, \text{s}^{-1} \]
Transcribed Image Text:**Problem: Calculate the Rate Constant** Calculate the rate constant, \( k \), for a reaction at 60.0 °C that has an activation energy of 77.7 kJ/mol and a frequency factor of \( 6.59 \times 10^{11} \, \text{s}^{-1} \). **Solution:** To calculate the rate constant \( k \), use the Arrhenius equation: \[ k = A e^{-\frac{E_a}{RT}} \] where: - \( k \) is the rate constant, - \( A \) is the frequency factor (\( 6.59 \times 10^{11} \, \text{s}^{-1} \)), - \( E_a \) is the activation energy (77.7 kJ/mol), - \( R \) is the gas constant (8.314 J/(mol·K)), - \( T \) is the temperature in Kelvin (60.0 °C = 333.15 K). Enter the calculated value of \( k \) in the provided box: \[ k = \_\_\_\_\_\_\_\_\_\_ \, \text{s}^{-1} \]
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