1. What is Arrhenius Constant for Zero Order Reaction?

Definition: The Arrhenius constant (A), also called the frequency factor, represents the frequency of collisions between reactant molecules with proper orientation for reaction.

Purpose: It's a key parameter in the Arrhenius equation that helps predict reaction rates at different temperatures.

2. How Does the Calculator Work?

The calculator uses the Arrhenius equation for zero-order reactions:

Where:

• \( A \) — Arrhenius constant (frequency factor)
• \( k_0 \) — Rate constant for zero-order reaction (mol/m³·s)
• \( E_a \) — Activation energy (J/mol)
• \( R \) — Universal gas constant (8.314 J/mol·K)
• \( T \) — Absolute temperature (K)

Explanation: The equation relates the reaction rate constant to temperature and activation energy.

3. Importance of Arrhenius Constant

Details: The Arrhenius constant helps predict how reaction rates change with temperature and is essential for reaction kinetics studies.

4. Using the Calculator

Tips: Enter the rate constant (k₀), activation energy (Eₐ) in J/mol, and temperature in Kelvin. All values must be > 0.

5. Frequently Asked Questions (FAQ)

Q1: What's the difference between A and k₀?
A: A is the frequency factor (maximum possible rate), while k₀ is the actual rate constant at a specific temperature.

Q2: What are typical units for A?
A: For zero-order reactions, A typically has units of mol/m³·s (same as the rate constant).

Q3: How does temperature affect A?
A: The Arrhenius constant A is theoretically temperature-independent, though in practice it may vary slightly.

Q4: What's a typical value for A?
A: Values vary widely, from 10⁶ to 10¹⁴ for different reactions, depending on molecular complexity.

Q5: Why is this specific to zero-order reactions?
A: While the Arrhenius form is similar for all orders, the units and interpretation of A differ by reaction order.