1. What is the Arrhenius Equation?

The Arrhenius equation describes the temperature dependence of reaction rates. It relates the rate constant (k) of a chemical reaction to the temperature (T), activation energy (Ea), and pre-exponential factor (A).

2. How Does the Calculator Work?

The calculator uses the Arrhenius equation:

Where:

• \( k \) — Rate constant (1/s)
• \( A \) — Pre-exponential factor (1/s)
• \( E_a \) — Activation energy (J/mol)
• \( R \) — Universal gas constant (8.314 J/mol K)
• \( T \) — Absolute temperature (K)

Explanation: The equation shows how the rate constant increases with temperature and decreases with higher activation energy.

3. Importance of Rate Constant Calculation

Details: The rate constant is fundamental in chemical kinetics, used to predict reaction rates under different conditions and design chemical processes.

4. Using the Calculator

Tips: Enter the pre-exponential factor in 1/s, activation energy in J/mol, and temperature in Kelvin. All values must be positive.

5. Frequently Asked Questions (FAQ)

Q1: What are typical values for the pre-exponential factor?
A: For simple reactions, A is typically 10^10 to 10^13 1/s, but can vary widely depending on the reaction.

Q2: How does temperature affect the rate constant?
A: Generally, increasing temperature increases the rate constant exponentially, as described by the Arrhenius equation.

Q3: What is the significance of activation energy?
A: Activation energy represents the minimum energy required for a reaction to occur. Higher Ea means slower reaction at a given temperature.

Q4: Can this equation be used for all reactions?
A: The Arrhenius equation works well for elementary reactions but may need modification for complex reactions.

Q5: Why use Kelvin for temperature?
A: The Arrhenius equation requires absolute temperature to properly account for the exponential relationship between temperature and reaction rate.