5. From the activation energy (Ea) and collision frequency factor (A) that you determined in this experiment, calculate the rate constant at 85 degrees Celsius.

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The activasion energy is -9.590 KJ/mol

The collision frequency is 7.05x10^8

 

 

**Question 5: Calculation of Rate Constant Using Arrhenius Equation**

From the activation energy (Ea) and collision frequency factor (A) that you determined in this experiment, calculate the rate constant at 85 degrees Celsius.

**Instruction:**

To complete this calculation, use the Arrhenius equation given by:

\[ k = A \cdot e^{-\frac{E_a}{RT}} \]

Where:
- \( k \) is the rate constant.
- \( A \) is the collision frequency factor.
- \( E_a \) is the activation energy.
- \( R \) is the universal gas constant (\( 8.314 \, \text{J/mol·K} \)).
- \( T \) is the temperature in Kelvin.

Here, convert the temperature from Celsius to Kelvin using the formula:
\[ T(K) = T(°C) + 273.15 \]

For 85 degrees Celsius:
\[ T = 85 + 273.15 = 358.15 \, \text{K} \]

Substitute the values of \( A \), \( E_a \), \( R \), and \(T \) into the Arrhenius equation to determine the rate constant \( k \).
Transcribed Image Text:**Question 5: Calculation of Rate Constant Using Arrhenius Equation** From the activation energy (Ea) and collision frequency factor (A) that you determined in this experiment, calculate the rate constant at 85 degrees Celsius. **Instruction:** To complete this calculation, use the Arrhenius equation given by: \[ k = A \cdot e^{-\frac{E_a}{RT}} \] Where: - \( k \) is the rate constant. - \( A \) is the collision frequency factor. - \( E_a \) is the activation energy. - \( R \) is the universal gas constant (\( 8.314 \, \text{J/mol·K} \)). - \( T \) is the temperature in Kelvin. Here, convert the temperature from Celsius to Kelvin using the formula: \[ T(K) = T(°C) + 273.15 \] For 85 degrees Celsius: \[ T = 85 + 273.15 = 358.15 \, \text{K} \] Substitute the values of \( A \), \( E_a \), \( R \), and \(T \) into the Arrhenius equation to determine the rate constant \( k \).
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