1. What is Rate Constant for Zero Order Reaction?

Definition: The rate constant for a zero-order reaction is equal to the rate of the reaction because in a zero-order reaction, the rate is independent of the concentration of the reactant.

Purpose: This calculator determines the rate constant using the Arrhenius equation, which relates reaction rates to temperature.

2. How Does the Calculator Work?

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

Where:

• \( k_0 \) — Rate constant for zero-order reaction (mol/(m³·s))
• \( A_{zero} \) — Frequency factor (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 shows how the rate constant increases with temperature and decreases with higher activation energy.

3. Importance of Rate Constant Calculation

Details: Knowing the rate constant helps predict reaction rates, design chemical processes, and understand reaction mechanisms.

4. Using the Calculator

Tips: Enter the frequency factor (pre-exponential factor), activation energy in J/mol, and temperature in Kelvin. All values must be > 0.

5. Frequently Asked Questions (FAQ)

Q1: What is the frequency factor (A)?
A: It represents the frequency of collisions with proper orientation for reaction to occur.

Q2: What are typical activation energy values?
A: Typically ranges from 50-250 kJ/mol for many chemical reactions.

Q3: Why does temperature affect the rate constant?
A: Higher temperature increases molecular collisions and the fraction of molecules with sufficient energy to overcome the activation barrier.

Q4: What's the difference between zero-order and other reaction orders?
A: In zero-order reactions, the rate is independent of reactant concentration, unlike first or second-order reactions.

Q5: Can this calculator be used for other reaction orders?
A: No, this is specific for zero-order reactions. Other orders have different Arrhenius equation forms.