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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.
The calculator uses the Arrhenius equation for zero-order reactions:
Where:
Explanation: The equation shows how the rate constant increases with temperature and decreases with higher activation energy.
Details: Knowing the rate constant helps predict reaction rates, design chemical processes, and understand reaction mechanisms.
Tips: Enter the frequency factor (pre-exponential factor), activation energy in J/mol, and temperature in Kelvin. All values must be > 0.
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.